All categories

3 years ago

20 mL of 80°C water is mixed with 20 mL of 0°C water in a perfect calorimeter. What is the final temperature?

1 answer:

8 0

To calculate for the final temperature, we need to remember that the heat rejected should be equal to the absorbed by the other system. We calculate as follows:

Q1 = Q2
(mCΔT)1 = (mCΔT)2

We can cancel m assuming the two systems are equal in mass. Also, we cancel C since they are the same system. This leaves us,

(ΔT)1 = (ΔT)2
(T - 80) = (0 - T)
T = 40°C

You might be interested in

What are the products formed when zinc reacts to dilute hydrochloride acid

joja [24]

The formula is:

Zn + Hcl —> H2 +Zncl2

Hence, the 2 products formed are:
Hydrogen gas and salt

Hope it helps!

5 0

3 years ago

Read 2 more answers

What form of heat transfer makes warm air rise?

zlopas [31]

Convection which allows heat to be transferred between the air molecule via convection currents .

3 0

3 years ago

( HELP) The following system is at equilibrium. In which direction (right or left) will the equilibrium position shift with the

Alex Ar [27]

a) right

b) left

c) left

d) right

e) right

f) no effect

d) left

Explanation:

We have the following chemical reaction:

3 NO (g) ⇔ N₂O (g) + NO₂ (g) + 154.9 kJ

a) right, because by lowering the temperature you remove the heat generated by the reaction, and the reaction is able to generate more heat with the reaction proceeding from left to right.

b) left, because by increasing the temperature you add heat to the reaction and by doing so the reaction from right to left will be promoted.

c) left, increasing the concentration of N₂O the equilibrium will shift to left in order to consume the N₂O added.

d) right, increasing the concentration of NO the equilibrium will shift to right in order to consume the NO added.

e) right, decreasing the concentration of N₂O the equilibrium will shift to right in order to produce the removed N₂O.

f) no effect, adding a catalyst will not shift the equilibrium position, it will only modify the time in which the equilibrium is achieved and the energy required to achieve the equilibrium state.

g) left, by increasing the volume the equilibrium will shift to the part where more moles are produced (there are 3 moles on left side while in the right side there are 2 moles).

Learn more about:

Le Chatelier Principle

brainly.com/question/4356622

brainly.com/question/3160814

#learnwithBrainly

8 0

4 years ago

Which of the following concerning the effects of temperature and pressure on solubility is/are correct?

just olya [345]

Answer:

None of the options are correct.

Explanation:

1) when the temperature of the solution is increased the solubility of the gas in the liquid decreases , hence option 1 is incorrect.

2)The heat released by the dissolution of an ionic compound in water is heat of hydration of the compound and is independent of the initial temperature of the solution.

3) The solubility of a liquid in water is not affected significantly by the pressure changes in the system as gases only have a significant cahne in solubility with change in pressure.

5 0

3 years ago

If 5.4 moles of Fe react with 4.7 moles of O2, what is the maximum amount of Fe2O3 (in moles) that can be produced? What is the

DIA [1.3K]

Answer:

2.7 moles of Fe₂O₃ is the maximum amount that can be produced. Iron is the limiting reactant.

Explanation:

The balanced reaction is:

4 Fe + 3 O₂ → 2 Fe₂O₃

By reaction stoichiometry (that is, the relationship between the amount of reagents and products in a chemical reaction), the following amounts of each compound participate in the reaction:

Fe: 4 moles
O₂: 3 moles
Fe₂O3: 2 moles

The limiting reagent is one that is consumed first in its entirety, determining the amount of product in the reaction. When the limiting reagent is finished, the chemical reaction will stop.

You can use a simple rule of three as follows: if by stoichiometry 4 moles of Fe reacts with 3 moles of O₂, how much moles of Fe will be needed if 4.7 moles of O₂ react?

$moles of Fe =\frac{4. moles of Fe*4.7 moles of O_{2}}{3 moles of O_{2} }$

moles of O₂= 6.27

But 6.27 moles of Fe are not available, 5.4 moles are available. Since you have less moles than you need to react with 4.7 moles of O₂, iron Fe will be the limiting reagent.

So you can use a simple rule of three as follows: if by stoichiometry 4 moles of Fe produce 2 moles of Fe₂O₃, how many moles of Fe₂O₃ will be produced if 5.4 moles of Fe react?

$moles of Fe_{2}O_{3}=\frac{5.4 moles of Fe*2 moles of Fe_{2} O_{3} }{4 moles of Fe}$

moles of Fe₂O₃= 2.7 moles

Then:

<u><em>2.7 moles of Fe₂O₃ is the maximum amount that can be produced. Iron is the limiting reactant.</em></u>

4 0

3 years ago