Can someone check and make sure I'm doing these problems right? Thanks so much!!
1. N2 + 3H2 ==> 2NH3 : How many moles of hydrogen are needed to completely react with two moles of nitrogen?
==> I got 6 moles.
3. Zn + 2HCl ==> ZnCl2 + H2 : How many moles of hydrogen are produced from the reaction of three moles of zinc with an excess of hydrochloric acid?
==> I got 3 moles.
5. K3PO4 + Al(NO3)3 ==> 3KNO3 + AlPO4 : How many moles of potassium nitrate are produced when two moles of potassium phosphate react with two moles of aluminum nitrate?
==> I got 6 moles.
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These problems are mass-mass problems:
1. 2KClO3 ==> 2KCl + 3O2 : How many grams of potassium chloride are produced if 25 g of potassium chlorate decompose?
==> I got 15.16 grams.
2. N2 + 3H2 ==> 2NH3 : How many grams of hydrogen are necessary to react completely with 50 g of nitrogen in the above reaction?
==> I got 10.71 g.
56767tyty
To check your answers for each problem, let's go through the calculations step by step:
1. N2 + 3H2 ==> 2NH3 : How many moles of hydrogen are needed to completely react with two moles of nitrogen?
The balanced equation tells us that 1 mole of nitrogen reacts with 3 moles of hydrogen. To find out how many moles of hydrogen are needed for 2 moles of nitrogen, we can set up a ratio:
2 moles of nitrogen * (3 moles of hydrogen / 1 mole of nitrogen) = 6 moles of hydrogen
So the correct answer is indeed 6 moles.
3. Zn + 2HCl ==> ZnCl2 + H2 : How many moles of hydrogen are produced from the reaction of three moles of zinc with an excess of hydrochloric acid?
Using the balanced equation, we see that 1 mole of zinc reacts with 2 moles of hydrochloric acid to produce 1 mole of hydrogen. Therefore, for 3 moles of zinc, we have:
3 moles of zinc * (2 moles of HCl / 1 mole of zinc) * (1 mole of hydrogen / 2 moles of HCl) = 3 moles of hydrogen
So your answer of 3 moles is correct.
5. K3PO4 + Al(NO3)3 ==> 3KNO3 + AlPO4 : How many moles of potassium nitrate are produced when two moles of potassium phosphate react with two moles of aluminum nitrate?
According to the balanced equation, 1 mole of potassium phosphate produces 3 moles of potassium nitrate. Therefore, for 2 moles of potassium phosphate, we have:
2 moles of potassium phosphate * (3 moles of KNO3 / 1 mole of K3PO4) = 6 moles of potassium nitrate
Your answer of 6 moles is correct.
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Mass-mass problems:
1. 2KClO3 ==> 2KCl + 3O2 : How many grams of potassium chloride are produced if 25 g of potassium chlorate decompose?
To solve this problem, we need to use the molar mass of potassium chlorate (2KClO3). The molar mass of KClO3 can be calculated as follows:
2 moles of potassium (2 x 39.10 g/mol) + 1 mole of chlorine (1 x 35.45 g/mol) + 3 moles of oxygen (3 x 16.00 g/mol) = 122.55 g/mol
Now, we can set up a ratio to find the number of moles of potassium chlorate:
25 g of KClO3 * (1 mole of KClO3 / 122.55 g of KClO3) = 0.204 moles of KClO3
From the balanced equation, we know that 2 moles of KClO3 produce 2 moles of KCl. Therefore, 0.204 moles of KClO3 will produce:
0.204 moles of KClO3 * (2 moles of KCl / 2 moles of KClO3) = 0.204 moles of KCl
To find the mass of KCl produced, we can use the molar mass of KCl (39.10 g/mol):
0.204 moles of KCl * (39.10 g of KCl / 1 mole of KCl) = 7.98 grams of KCl
So the correct answer is approximately 7.98 grams.
2. N2 + 3H2 ==> 2NH3 : How many grams of hydrogen are necessary to react completely with 50 g of nitrogen?
First, we need to find the number of moles of nitrogen using its molar mass (28.02 g/mol):
50 g of N2 * (1 mole of N2 / 28.02 g of N2) = 1.785 moles of N2
Using the balanced equation, we know that 3 moles of H2 react with 1 mole of N2 to produce 2 moles of NH3. Therefore, for 1.785 moles of N2, we have:
1.785 moles of N2 * (3 moles of H2 / 1 mole of N2) = 5.355 moles of H2
Finally, we can find the mass of hydrogen by multiplying the number of moles by its molar mass (2.02 g/mol):
5.355 moles of H2 * (2.02 g of H2 / 1 mole of H2) = 10.84 grams of H2
So the correct answer is approximately 10.84 grams.