Answer:
Step-by-step explanation:
First, we need to calculate the number of moles of CuO present in the reaction:
Number of moles = mass / molar mass
Number of moles of CuO = 14.4 mol x (1 mol CuO / 3 mol CuO) = 4.8 mol CuO
Using the stoichiometry of the balanced equation, we know that for every 3 moles of CuO consumed, we can produce 1 mole of N2. Therefore:
Number of moles of N2 = 4.8 mol CuO x (1 mol N2 / 3 mol CuO) = 1.6 mol N2
To calculate the mass of N2 produced, we use the molar mass of nitrogen:
Mass of N2 = number of moles x molar mass = 1.6 mol x 28 g/mol = 44.8 g
Rounding to the nearest tenth, the answer is 44.8 grams of N2 produced.
The balanced equation tells us that one mole of carbon reacts with two moles of hydrogen gas to produce one mole of methane. Therefore, we need to use a ratio to find the amount of carbon needed to produce 19.5 moles of methane:
19.5 mol CH4 x (1 mol C / 1 mol CH4) = 19.5 mol C
To convert moles of carbon to grams, we use the molar mass of carbon:
19.5 mol C x 12 g/mol = 234 g
Rounding to the nearest tenth, the answer is 234.0 grams of carbon needed.
We can start by calculating the number of moles of methane present:
Number of moles = mass / molar mass
Number of moles of CH4 = 119.4 g / 16 g/mol = 7.46 mol
From the balanced equation, we know that one mole of carbon reacts with two moles of hydrogen gas to produce one mole of methane. Therefore:
Number of moles of C = 7.46 mol CH4 x (1 mol C / 1 mol CH4) = 7.46 mol C
Rounding to the nearest tenth, the answer is 7.5 moles of carbon needed.
First, we need to calculate the number of moles of CuO present in the reaction:
Number of moles = mass / molar mass
Number of moles of CuO = 127.4 g / 79.5 g/mol = 1.6 mol CuO
Using the stoichiometry of the balanced equation, we know that for every 3 moles of CuO consumed, we can produce 1 mole of N2. Therefore:
Number of moles of N2 = 1.6 mol CuO x (1 mol N2 / 3 mol CuO) = 0.53 mol N2
Rounding to the nearest tenth, the answer is 0.5 moles of N2 produced.