What is the energy required to go from a solid to a liquid called?

Cell Structure and Functions Activity Worksheet

ICE Princess25 [194]

Answer:

u still need this?

Explanation:

4 0

3 years ago

Read 2 more answers

Which parameter is indicative of how far and in what direction a reaction will progress?

nekit [7.7K]

Answer:

Option b, The change in free energy of the reaction (ΔG)

Explanation:

Gibbs free energy is a measure of amount of usable energy in the system.

It is related with enthalpy (H), entropy (S) and temprature (T) as:

G = H - TS

The Gibbs free energy change (ΔG) provide spontaneity of a chemical reaction.

If ΔG is negative, then reaction is spontaneous that means reaction is moving towards forward direction.

If ΔG is positive, then reaction is non-spontaneous that means reaction is moving in backward direction.

If ΔG is zero, then reaction is at equilibrium.

Change in enthalpy only gives informtion about heat involed in a chemical reaction, it does not give information about direction of the reaction.

So, among the given options, option b is correct.

6 0

3 years ago

Could someone please help!

bezimeni [28]

Im pretty sure that the current will increase so the answer is A . Hope that helps

8 0

3 years ago

3. A compound was analyzed and found to contain 9.8 g of nitrogen, 0.70 g of

Nesterboy [21]

Answer:

HNO₃

Explanation:

Data given

Nitrogen = 9.8 g

Hydrogen = 0.70 g

Oxygen = 33.6 g

Empirical formula = ?

Solution:

Convert the masses to moles

For Nitrogen

Molar mass of N = 14 g/mol

no. of mole = mass in g / molar mass

Put value in above formula

no. of mole = 9.8 g/ 14 g/mol

no. of mole = 0.7

mole of N = 0.7 mol

For Hydrogen

Molar mass of H = 1 g/mol

no. of mole = mass in g / molar mass

Put value in above formula

no. of mole = 0.70 g/ 1 g/mol

no. of mole = 0.7

mole of H = 0.7 mol

For Oxygen

Molar mass of O = 16 g/mol

no. of mole = mass in g / molar mass

Put value in above formula

no. of mole = 33.6 g / 16 g/mol

no. of mole = 2.1

mole of O = 2.1 mol

Now we have values in moles as below

N = 0.7

H = 0.7

O = 2.1

Divide the all values on the smallest values to get whole number ratio

N = 0.7 / 0.7 = 1

H = 0.7 / 0.7 = 1

O = 2.1 / 0.7 = 3

So all have following values

N = 1

H = 1

O = 3

So the empirical formula will be HNO₃ i.e. all three atoms in simplest small ratio.

6 0

3 years ago

How many grams of K2O will be produced from 0.50 g of K<br> and 0.10 g of O2?

Rudik [331]

Answer:

0.6g

Explanation:

Given parameters:

Mass of K = 0.5g

Mass of O₂ = 0.10g

Unknown:

Mass of K₂O = ?

Solution:

To solve this problem, let us write the reaction equation first;

4K + O₂ → 2K₂O

The reaction above delineates the balanced chemical reaction.

To solve this problem, we need to know the limiting reactant. This reactant is the one that determines the amount and extent of the reaction because it is given in short supply. The other reactant is the one in excess.

Start off by find the number of moles of the reactant;

Number of moles = $\frac{mass}{molar mass}$

Molar mas of K = 39g/mol

Molar mass of O₂ = 2(16) = 32g/mol

Number of moles of K = $\frac{0.5}{39}$ = 0.013moles

Number of moles of O₂ = $\frac{0.1}{32}$ = 0.031moles

From the balanced reaction;

4 moles of K reacted with 1 mole of O₂

0.013 moles of K will react with $\frac{0.013}{4}$ = 0.0078 moles of O₂

We see that oxygen gas is in excess. We were given 0.031moles of the gas but only require 0.0078moles of oxygen gas.

The limiting reactant is potassium.

therefore;

4 moles of K produced 2 moles of K₂O

0.013 moles of K will produce $\frac{0.013 x 2}{4}$ = 0.0065‬moles of K₂O

to find the mass of K₂O;

Mass of K₂O = number of moles x molar mass

Molar mass of K₂O = 2(39) + 16 = 94g/mol

Mass of K₂O = 0.0065 x 94 = 0.6g

7 0

3 years ago