We calculate for the number of moles of water given its mass by dividing the given mass by the molar mass.
n water = (36.04 g) / (18 g/mol)
n water = 2 mols
From the given balanced equation, every 6 moles of water produced will require 7 moles of oxygen.
n oxygen = (2 mols H2O) x (7 moles O2 / 6 moles H2O)
n oxygen = 2.33 mols O2
Answer:
As2O3 → H3AsO4
As2O3 → 2H3AsO4 balance As
5H2O + As2O3 → 2H3AsO4 balance O by adding H2O to one side
5H2O + As2O3 → 2H3AsO4 + 4H+ balance H by adding H+ to one side
5H2O + As2O3 → 2H3AsO4 + 4 H+ + 4e- balance charge by adding electrons to one side
Now do the same for the other part of the reaction
NO3- → NO
NO3- → NO + 2H2O
4H+ + NO3- → NO + 2H2O
3e- + 4H+ + NO3- → NO + 2H2O
Now cancel the electrons by multiplying the first equation by 3 and the second equation by 4, then add them together
.
3As2O3 + 4NO3- + 7H2O + 4H+ → 6H3AsO4 + 4NO
Answer:
55.0 g
Explanation:
Step 1: Write the balanced equation for the production of oxygen
2 CO₂(g)⇒ 2 CO(g) + O₂(g)
Step 2: Calculate the mass of oxygen produced over a 2 hour period
The MOXIE produces 10.0 g of oxygen per hour.
2 h × 10.0 g/1 h = 20.0 g
Step 3: Calculate the moles corresponding to 20.0 g of O₂
The molar mass of O₂ is 32.00 g/mol.
20.0 g × 1 mol/32.00 g = 0.625 mol
Step 4: Calculate the number of moles of CO₂ needed to produce 0.625 moles of O₂
The molar ratio of CO₂ to O₂ is 2:1. The moles of CO₂ needed are 2/1 × 0.625 mol = 1.25 mol
Step 5: Calculate the mass corresponding to 1.25 moles of CO₂
The molar mass of CO₂ is 44.01 g/mol.
1.25 mol × 44.01 g/mol = 55.0 g
Answer:
32.0 kJ
General Formulas and Concepts:
<u>Thermochemistry</u>
Specific Heat Formula: q = mcΔT
- q is heat (in J)
- m is mass (in g)
- c is specific heat (in J/g °C)
- ΔT is change in temperature (in °C)
Explanation:
<u>Step 1: Define</u>
<em>Identify variables</em>
[Given] <em>m</em> = 1.00 g
[Given] ΔT = 1.48 °C
[Given] <em>c</em> = 21.6 kJ/g °C
[Solve] <em>q</em>
<em />
<u>Step 2: Find Heat</u>
- Substitute in variables [Specific Heat Formula]: q = (1.00 g)(21.6 kJ/g °C)(1.48 °C)
- Multiply [Cancel out units]: q = (21.6 kJ/°C)(1.48 °C)
- Multiply [Cancel out units]: q = 31.968 kJ
<u>Step 3: Check</u>
<em>Follow sig fig rules and round. We are given 3 sig figs.</em>
31.968 kJ ≈ 32.0 kJ