how many kilograms of NH3 are needed to produce 2.90x10^5kg of (NH4)2SO4?

the balanced equation is:
2 NH3 + H2SO4 --> (NH4)2SO4

1. Convert 2.90x10^5kg of (NH4)2SO4 to kilogram•moles by dividing by 132.26 kg/kg.mol

2. Since 2 kg.moles of NH3 produces 1 kg.mole of (NH4)2SO4, multiply the answer to Step 1 by 2 to get kg.moles of NH3 needed.

3. multiply the previous answer by 17.09 kg/kg.mol of NH3 to get kgs of NH3 needed.

To find out how many kilograms of NH3 are needed to produce 2.90x10^5 kg of (NH4)2SO4, we first need to determine the molar ratio between NH3 and (NH4)2SO4.

According to the balanced equation:
2 NH3 + H2SO4 → (NH4)2SO4

The molar ratio between NH3 and (NH4)2SO4 is 2:1. This means that for every 2 moles of NH3, we can produce 1 mole of (NH4)2SO4.

To calculate the amount of NH3 needed, we can use the following steps:

1. Determine the molar mass of (NH4)2SO4:
(NH4)2SO4 = 2(NH4) + SO4 = 2(14.01 g/mol) + 32.06 g/mol = 132.14 g/mol

2. Convert the given mass of (NH4)2SO4 to moles:
2.90x10^5 kg x (1000 g/1 kg) x (1 mol/132.14 g) = approximately 2196 mol

3. Use the molar ratio to find the required amount of NH3:
mols of NH3 = 1/2 x mols of (NH4)2SO4
mols of NH3 = 1/2 x 2196 mol = 1098 mol

4. Convert moles of NH3 to kilograms:
1098 mol x 17.03 g/mol x (1 kg/1000 g) = approximately 18.7 kg

Therefore, 18.7 kilograms of NH3 are needed to produce 2.90x10^5 kilograms of (NH4)2SO4.