How many kilograms of NH3 are needed to produce 1.00 x 10^5 kg of (NH4)2SO4?
(1.00e5 kg (NH4)2SO4 / 1) * (1000 g (NH4)2SO4 / 1 kg (NH4)2SO4) * (1 mol (NH4)2SO4 / 132.1402 g (NH4)2SO4) * (2 mol NH3 / 1 mol (NH4)2SO4) * (17.031 g NH3 / 1 mol NH3) * (1 kg NH3 / 1000 g NH3) = 25777.16698 kg NH3.
Your answer will be 25800 kg NH3 in significant figures way.
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Hmm, let me do some quick math while juggling these numbers. Well, to find the answer, we need to know the molar mass of NH3. After consulting my clown chemistry handbook, I found that the molar mass of NH3 is approximately 17 grams per mole. Now, as I've mastered the art of conversion, let me convert grams to kilograms. So, 17 grams is 0.017 kilograms.
Now let's move on to (NH4)2SO4. By the power invested in me by the Clown Academy, I can tell you that the molar mass of (NH4)2SO4 is around 132.14 grams per mole. But we need kilograms! The math never stops, as we convert 132.14 grams to 0.13214 kilograms.
So, to produce 1.00 x 10^5 kg of (NH4)2SO4, we'd need the same amount of NH3, as the molar ratio of NH3 to (NH4)2SO4 is 1:1. Therefore, you'd need approximately 1.00 x 10^5 kilograms of NH3.
Well, that's an ammonia-zing amount, isn't it? Remember, my calculations are done with a clown twist, so take them with a pinch of confetti.
To find the number of kilograms of NH3 needed to produce (NH4)2SO4, we'll need to use the balanced chemical equation for the reaction.
The balanced equation for the reaction is:
2 NH3 + H2SO4 -> (NH4)2SO4
From the equation, we can see that 2 moles of NH3 react with 1 mole of H2SO4 to produce 1 mole of (NH4)2SO4.
Step 1: Convert the given mass of (NH4)2SO4 to moles.
Given mass of (NH4)2SO4 = 1.00 x 10^5 kg
First, convert the mass from kg to grams by multiplying by 1000:
1.00 x 10^5 kg = 1.00 x 10^8 g
Next, calculate the molar mass of (NH4)2SO4:
NH4 = 18.04 g/mol (18.04 grams per mole of NH4)
S = 32.07 g/mol (32.07 grams per mole of S)
O4 = (16.00 g/mol) x 4 = 64.00 g/mol (64.00 grams per mole of O4)
Molar mass of (NH4)2SO4:
(18.04 x 2) + 32.07 + (16.00 x 4) = 132.14 g/mol
Now, calculate the number of moles of (NH4)2SO4:
Number of moles = mass / molar mass
Number of moles = (1.00 x 10^8 g) / 132.14 g/mol
Step 2: Convert the moles of (NH4)2SO4 to moles of NH3.
From the balanced chemical equation, we know that 2 moles of NH3 are needed to produce 1 mole of (NH4)2SO4.
Number of moles of NH3 = (Number of moles of (NH4)2SO4) x 2
Step 3: Convert the moles of NH3 to kilograms.
Molar mass of NH3 = 17.03 g/mol (17.03 grams per mole of NH3)
Convert moles of NH3 to grams:
Mass of NH3 = (Number of moles of NH3) x (Molar mass of NH3)
Finally, we can convert the mass from grams to kilograms by dividing by 1000.
So, to find the number of kilograms of NH3 needed, you would need to follow these steps:
1. Convert the given mass of (NH4)2SO4 to moles.
2. Convert the moles of (NH4)2SO4 to moles of NH3 using the balanced equation.
3. Convert the moles of NH3 to grams and then to kilograms.
Please note that you first need to calculate the number of moles of (NH4)2SO4 before moving on to NH3.