section 2\nproblems write the answer on the l...
section 2\nproblems write the answer on the line to the left. show all your work in the\nspace provided.\n1. the following equation represents a laboratory\npreparation for oxygen gas:\n2kclo₃(s) → 2kcl(s) + 3o₂(g)\nhow many moles of o₂ form if 3.0 mol of kclo₃ are\ntotally consumed?\n2. given the following equation:\nh₂(g) + f₂(g) → 2hf(g) how many grams of hf gas\nare produced as 5 mol of fluorine react?\n3. water can be made to decompose into its elements by\nusing electricity according to the following equation:\n2h₂o(l) → 2h₂(g) + o₂(g)\nhow many grams of o₂ are produced when 0.033\nmol of water decompose?\n4. sodium metal reacts with water to produce naoh\naccording to the following equation:\n2na(s) + 2h₂o(l) → 2naoh(aq) + h₂(g)\nhow many grams of naoh are produced if 20.0 g of\nsodium metal react with excess oxygen?
Answer
### Problem 1
# Explanation:
## Step1: Determine mole ratio
From the equation \(2KClO_3(s)\to2KCl(s) + 3O_2(g)\), the mole ratio of \(KClO_3\) to \(O_2\) is \(2:3\).
## Step2: Calculate moles of \(O_2\)
Let \(x\) be the moles of \(O_2\). Using the ratio \(\frac{2}{3}=\frac{3.0}{x}\), cross - multiply: \(2x = 3\times3.0\), so \(x=\frac{9.0}{2}=4.5\)
# Answer:
\(4.5\) mol
### Problem 2
# Explanation:
## Step1: Determine mole ratio
From the equation \(H_2(g)+F_2(g)\to2HF(g)\), the mole ratio of \(F_2\) to \(HF\) is \(1:2\). If \(n(F_2) = 5\) mol, then \(n(HF)=2\times5 = 10\) mol.
## Step2: Calculate mass of \(HF\)
The molar mass of \(HF\) is \(M(HF)=1 + 19=20\) g/mol. Using \(m = n\times M\), \(m(HF)=10\times20 = 200\) g
# Answer:
\(200\) g
### Problem 3
# Explanation:
## Step1: Determine mole ratio
From the equation \(2H_2O(l)\to2H_2(g)+O_2(g)\), the mole ratio of \(H_2O\) to \(O_2\) is \(2:1\). If \(n(H_2O)=0.033\) mol, then \(n(O_2)=\frac{0.033}{2}=0.0165\) mol.
## Step2: Calculate mass of \(O_2\)
The molar mass of \(O_2\) is \(M(O_2)=32\) g/mol. Using \(m=n\times M\), \(m(O_2)=0.0165\times32 = 0.528\) g
# Answer:
\(0.528\) g
### Problem 4
# Explanation:
## Step1: Calculate moles of \(Na\)
The molar mass of \(Na\) is \(M(Na) = 23\) g/mol. \(n(Na)=\frac{20.0}{23}\) mol.
## Step2: Determine mole ratio
From the equation \(2Na(s)+2H_2O(l)\to2NaOH(aq)+H_2(g)\), the mole ratio of \(Na\) to \(NaOH\) is \(1:1\). So \(n(NaOH)=\frac{20.0}{23}\) mol.
## Step3: Calculate mass of \(NaOH\)
The molar mass of \(NaOH\) is \(M(NaOH)=40\) g/mol. Using \(m = n\times M\), \(m(NaOH)=\frac{20.0}{23}\times40=\frac{800}{23}\approx34.8\) g
# Answer:
\(\approx34.8\) g