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Arada [10]
3 years ago
5

The primary method in which two connected objects transfer energy by heat flow is _____.

Chemistry
2 answers:
swat323 years ago
7 0
 Conduction is heat tranfer through physical contact. Hope this helps. :)
kramer3 years ago
5 0
The primary method in which two connected objects transfer energy by heat flow is conduction.
You might be interested in
for the reaction 2Fe + O2 = 2FeO, how many grams of iron oxide are produced from 8.00 mol of iron? when o2 is an excess
Luba_88 [7]

Answer:

2Fe + O₂ -------------------> 2FeO

8 mol Fe produce

8 mol Fe * 2 mol FeO / 2 mol Fe = 8 mol FeO

Mass of FeO = 8 mol FeO * 71.85 g/mol = 574.8 grams FeO

Explanation:

Having 8 mol of Iron means 8 moles of iron oxide can be produced. Each mole of iron oxide has a molecular weight of 71.85 grams. Therefore, 8 moles of iron oxide should weight 574.8 grams.

7 0
3 years ago
Will mark branliest. Calculating percent yield: For the reaction Cu + 2AgNO3 → Cu(NO3)2 + 2 Ag, adding 127 grams of copper to lo
pishuonlain [190]

Percent yield = (Actual Yield/ Theoretical Yield) x 100

Given, Actual Yield of silver = 410 grams

Given, mass of copper = 127 g

Atomic mass of copper = 63.546 amu

Formula: Moles = mass / atomic mass

Moles of copper = 127 g/ 63.546 amu = 1.998 mol

Based on the given balanced chemical reaction, the molar ratio between Cu: Ag is 1:2

So 1.998 mol of copper should yield (2 mol Ag/ 1 mol Cu) x 1.998 mol of Cu = 3.996 mol

Calculated mol of Ag = 3.996 mol

Atomic mass of silver = 107.8682 amu

Mass of silver = moles x atomic mass = 3.996 mol x 107.8682 amu = 431 g

Based on the math, the theoretical yield = 431 g

Percent yield of silver = (410g/431g) x 100 = 95. 13%

The answer is 95. 13%

8 0
3 years ago
Help me on this question, will give brainliest.
JulsSmile [24]
The answer is to this question is c
6 0
3 years ago
4-methyl-3-hexanol was prepared by reacting an alkene with either hydroboration-oxidation or oxymercuration-reduction. Draw the
Ivenika [448]

Answer:

Structure in attachment.

Explanation:

The oxymercuration-demercuration of an asymmetric alkene usually produces the  Markovnikov orientation of an addition. The electrophile ⁺Hg(OAc), formed by the electrophile attack of the mercury ion, remains attached to least substituted group at the end of the double bond. This electrophile has a considerable amount of positive charge on its two  carbon atoms, but there is more positive charge on the more substituted carbon atom,  where it is more stable. The water attack occurs on this more electrophilic carbon, and the Markovnikov orientation occurs.

In hydroboration, borane adds to the double bond in one step. Boron is added to the less  hindered and less substituted carbon, and hydrogen is added to the more substituted carbon. The electrophilic boron atom adds to the less substituted end of the double bond, positioning the positive charge (and the hydrogen atom) at the more substituted end. The result is a product with the anti-Markovnikov orientation.

3 0
3 years ago
A chemical equilibrium between gaseous reactants and products is shown.
fenix001 [56]

Explanation:

Question 1:

It will shift toward the reactant side as there are a greater number of moles of gas on the reactant side.

Pressure changes only affects only equilibrium involving a gas or gases. An increase in pressure shifts the equilibrium in the direction of the reaction with lower volume.

                 N₂  + 3H₂   ⇆   2NH₃

                        4                  2

An increase in pressure will shift the equilibrium towards the product side.

If the pressure is decreased, equilibrium will shifts towards the side of the reactants. This is because the volume of the reactants are higher than that of the product.

Question 2:

True

Based on Le Chatelier's principle, an increase in temperature will shift the equilibrium position towards the products in an endothermic reaction.

An endothermic reaction is a reaction that absorbs heat from the surroundings.

A rise in temperature shifts equilibrium position to the direction that absorbs the heat and vice versa.

In an endothermic reaction, the forward reaction absorbs the heat and therefore equilibrium shifts towards the side of product.

Question 3:

Decreasing the pressure              A) Shift to the left

Adding hydrogen gas                   B) Shift to the right

Adding a catalyst                          C) No effect

                N₂  + 3H₂   ⇆   2NH₃

Pressure : Decreasing the pressure will shift the equilibrium position to the left. In reactions involving gases, increase in pressure favors the side with a lesser volume. An increase in pressure will favor the formation of ammonia as a product.

A decrease in pressure shifts the equilibrium to the left towards the side of high volume.

Concentration: addition of hydrogen gas will increase the concentration of the gas. An increase in concentration favors the side that uses up the specie and lowers it concentration.

If the concentration of hydrogen gas is increased the equilibrium will shift to the right to annul the concentration of reactants that has increased.

Catalyst: Catalysts have no effect on the position of chemical equilibrium. It only affects the rate at which equilibrium can be reached.

Question 4:

Adding more of gas C to the system

The change that would shift the equilibrium system to the left is by adding more of gas C to the system.

This will increase the concentration of gas C, in order to annul this, the equilibrium will shift to the left.

  • Heating the system will shift the equilibrium to the right
  • Increasing volume only affects purely gaseous reactions.
  • Removing some of gas C from the system shifts the equilibrium to the right.

Question 5:

Heating the system

This is an exothermic reaction because enthalpy change is negative. A rise in temperature shifts equilibrium position to the direction that absorbs heat.

In an exothermic reaction, heat is given off in the forward process. The reverse process is endothermic and heat is absorbed.

Therefore, heating the system will shift the equilibrium to the left and heat is absorbed.

Question 6:

This reaction is exothermic because the system shifted to the left on heating.

It is right to conclude that this reaction is exothermic because the system shifted to the left on heating .

Since the reaction turned dark brown on heating, it shows that more of the reactant Nitrogen dioxide gas was produced.

We can see that the reaction is exothermic in the forward process. An increase in temperature shifts equilibrium position backward to the side that absorbs the heat. This allows for the production of more nitrogen dioxide.

Question 7:

Shift it toward the reactants

A decrease in the concentration of the reactants shift the reaction towards the sides of the reactants.

An increase in concentration of a specie favors the direction that uses up that specie and lowers its concentration.

If the concentration of a specie on the reactant side is increased, equilibrium shifts to the right where more products are formed.

if we decrease the concentration of reactants, the products will be more concentrated and the equilibrium will shift to the left i.e the reactant side.

Learn more:

Equilibrium constant brainly.com/question/11126965

#learnwithBrainly

3 0
3 years ago
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