Question

1. 2 NH3 + 3 CuO → 3 Cu + N2 + 3 H2O

In the above equation, how many grams of N2 can be made when 14.4 moles of CuO are consumed?

Round your answer to the nearest tenth. If you answer is a whole number like 4, report the answer as 4.0

Use the following molar masses. If you do not use these masses, the computer will mark your answer incorrect.:

Element Molar Mass
Hydrogen 1
Nitrogen 14
Copper 63.5
Oxygen 16

2. For the reaction C + 2H2 → CH4, how many grams of carbon are required to produce 19.5 moles of methane, CH4 ?

Round your answer to the nearest tenth. If you answer is a whole number like 4, report the answer as 4.0

Use the following molar masses. If you do not use these masses, the computer will mark your answer incorrect.:

Element Molar Mass
Hydrogen 1
Carbon 12

3. For the reaction C + 2H2 → CH4, how many moles of carbon are needed to make 119.4 grams of methane, CH4 ?

Round your answer to the nearest tenth. If you answer is a whole number like 4, report the answer as 4.0

Use the following molar masses. If you do not use these masses, the computer will mark your answer incorrect.:

Element

Molar Mass

Hydrogen

1

Carbon

12

4. 2 NH3 + 3 CuO --> 3 Cu + N2 + 3 H2O

In the above equation how many moles of N2 can be made when 127.4 grams of CuO are consumed?

Round your answer to the nearest tenth. If you answer is a whole number like 4, report the answer as 4.0

Use the following molar masses. If you do not use these masses, the computer will mark your answer incorrect.:

Element

Molar Mass

Hydrogen

1

Nitrogen

14

Copper

63.5

Oxygen

16

Answer 1

Step-by-step explanation:

First, we need to find the limiting reactant between CuO and NH3. We can do this by calculating the moles of each reactant based on the given amount of CuO:

Moles of CuO = 14.4 mol CuO

Moles of NH3 = (2/3) x 14.4 mol CuO = 9.6 mol NH3

Since NH3 has a smaller mole value than CuO, it is the limiting reactant. Thus, we need to use the mole ratio between NH3 and N2 to find the moles of N2 produced:

Moles of N2 = (1/2) x 9.6 mol NH3 = 4.8 mol N2

Finally, we can use the molar mass of N2 to find the mass of N2 produced:

Mass of N2 = 4.8 mol N2 x 28 g/mol N2 = 134.4 g N2

Rounded to the nearest tenth, the answer is 134.4 g N2.

The balanced chemical equation tells us that 1 mole of carbon reacts with 2 moles of hydrogen to produce 1 mole of methane. Thus, we can use the mole ratio to find the moles of carbon needed:

Moles of C = 1/3 x 19.5 mol CH4 = 6.5 mol C

Finally, we can use the molar mass of carbon to find the mass of carbon needed:

Mass of C = 6.5 mol C x 12 g/mol C = 78 g C

Rounded to the nearest tenth, the answer is 78.0 g C.

We can use the molar mass of methane to convert the given mass to moles:

Moles of CH4 = 119.4 g CH4 / 16 g/mol CH4 = 7.5 mol CH4

Since the balanced chemical equation tells us that 1 mole of carbon reacts with 1 mole of methane, we need the same amount of moles of carbon:

Moles of C = 7.5 mol CH4

Rounded to the nearest tenth, the answer is 7.5 mol C.

Similar to the first question, we need to find the limiting reactant between CuO and NH3. We can do this by calculating the moles of each reactant based on the given mass of CuO:

Moles of CuO = 127.4 g CuO / 63.5 g/mol CuO = 2.0 mol CuO

Moles of NH3 = (2/3) x 2.0 mol CuO = 1.3 mol NH3

Since NH3 has a smaller mole value than CuO, it is the limiting reactant. Thus, we need to use the mole ratio between NH3 and N2 to find the moles of N2 produced:

Moles of N2 = (1/2) x 1.3 mol NH3 = 0.65 mol N2

Rounded to the nearest tenth, the answer is 0.7 mol N2.