1. 2kclo₃ → 2kcl + 3o₂
how many grams of potassium chloride are produced if 25 g of potassium chlorate decompose?
2. n₂ + 3h₂ → 2nh₃
how many grams of hydrogen are necessary to react completely with 50.0 g of nitrogen in the above reaction?
3. how many grams of ammonia are produced in the reaction in problem 2?
4. 2agno₃ + bacl₂ → 2agcl + ba(no₃)₂
how many grams of silver chloride are produced from 5.0 g of silver nitrate reacting with an excess of barium chloride?
5. how much barium chloride is necessary to react with the silver nitrate in problem 4?

Question

Accepted Answer

### Problem 1
# Explanation:
## Step1: Calculate molar mass
Molar mass of $KClO_3$: $39 + 35.5+3\times16=122.5\space g/mol$
Molar mass of $KCl$: $39 + 35.5 = 74.5\space g/mol$
## Step2: Find moles of $KClO_3$
Moles of $KClO_3=\frac{25\space g}{122.5\space g/mol}\approx0.204\space mol$
## Step3: Use mole ratio
From $2KClO_3
ightarrow2KCl + 3O_2$, mole ratio $KClO_3:KCl = 2:2 = 1:1$
Moles of $KCl = 0.204\space mol$
## Step4: Calculate mass of $KCl$
Mass of $KCl=0.204\space mol\times74.5\space g/mol\approx15.2\space g$

# Answer:
$15.2\space g$

### Problem 2
# Explanation:
## Step1: Calculate molar mass
Molar mass of $N_2$: $2\times14 = 28\space g/mol$
Molar mass of $H_2$: $2\times1=2\space g/mol$
## Step2: Find moles of $N_2$
Moles of $N_2=\frac{50.0\space g}{28\space g/mol}\approx1.79\space mol$
## Step3: Use mole ratio
From $N_2 + 3H_2
ightarrow2NH_3$, mole ratio $N_2:H_2=1:3$
Moles of $H_2 = 1.79\space mol\times3 = 5.37\space mol$
## Step4: Calculate mass of $H_2$
Mass of $H_2=5.37\space mol\times2\space g/mol = 10.7\space g$

# Answer:
$10.7\space g$

### Problem 3
# Explanation:
## Step1: Calculate molar mass
Molar mass of $N_2$: $28\space g/mol$
Molar mass of $NH_3$: $14 + 3\times1=17\space g/mol$
## Step2: Find moles of $N_2$
Moles of $N_2=\frac{50.0\space g}{28\space g/mol}\approx1.79\space mol$
## Step3: Use mole ratio
From $N_2 + 3H_2
ightarrow2NH_3$, mole ratio $N_2:NH_3 = 1:2$
Moles of $NH_3=1.79\space mol\times2 = 3.58\space mol$
## Step4: Calculate mass of $NH_3$
Mass of $NH_3=3.58\space mol\times17\space g/mol\approx60.9\space g$

# Answer:
$60.9\space g$

### Problem 4
# Explanation:
## Step1: Calculate molar mass
Molar mass of $AgNO_3$: $108+14 + 3\times16=170\space g/mol$
Molar mass of $AgCl$: $108 + 35.5=143.5\space g/mol$
## Step2: Find moles of $AgNO_3$
Moles of $AgNO_3=\frac{5.0\space g}{170\space g/mol}\approx0.0294\space mol$
## Step3: Use mole ratio
From $2AgNO_3 + BaCl_2
ightarrow2AgCl+Ba(NO_3)_2$, mole ratio $AgNO_3:AgCl = 2:2 = 1:1$
Moles of $AgCl = 0.0294\space mol$
## Step4: Calculate mass of $AgCl$
Mass of $AgCl=0.0294\space mol\times143.5\space g/mol\approx4.22\space g$

# Answer:
$4.22\space g$

### Problem 5
# Explanation:
## Step1: Calculate molar mass
Molar mass of $AgNO_3$: $170\space g/mol$
Molar mass of $BaCl_2$: $137+2\times35.5 = 208\space g/mol$
## Step2: Find moles of $AgNO_3$
Moles of $AgNO_3=\frac{5.0\space g}{170\space g/mol}\approx0.0294\space mol$
## Step3: Use mole ratio
From $2AgNO_3 + BaCl_2
ightarrow2AgCl+Ba(NO_3)_2$, mole ratio $AgNO_3:BaCl_2 = 2:1$
Moles of $BaCl_2=\frac{0.0294\space mol}{2}=0.0147\space mol$
## Step4: Calculate mass of $BaCl_2$
Mass of $BaCl_2=0.0147\space mol\times208\space g/mol\approx3.06\space g$

# Answer:
$3.06\space g$

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QUESTION IMAGE

Question

Explanation:

Problem 1

Step1: Calculate molar mass

Step2: Find moles of \(KClO_3\)

Step3: Use mole ratio

Step4: Calculate mass of \(KCl\)

Step1: Calculate molar mass

Step2: Find moles of \(N_2\)

Step3: Use mole ratio

Step4: Calculate mass of \(H_2\)

Step1: Calculate molar mass

Step2: Find moles of \(N_2\)

Step3: Use mole ratio

Step4: Calculate mass of \(NH_3\)

Answer:

Problem 2