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zysi [14]
3 years ago
14

When 3.0 mol Al react with 7.0 mol HCl, what is the limiting reactant and how many moles of H2 can be formed?

Chemistry
1 answer:
inysia [295]3 years ago
6 0
HCl is the limiting reactant, and 3.5 mol H2<span> can be formed</span>
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Chemical i pretty sure! please do more searching if u think i’m wrong.
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A 1.00 L flask is filled with 1.10 g of argon at 25 ∘C. A sample of ethane vapor is added to the same flask until the total pres
Alex Ar [27]

Answer: a) Partial pressure of argon is 0.673 atm.

b) Partial pressure of ethane is 0.427 atm.

Explanation:

According to the ideal gas equation:'

PV=nRT

P = Pressure of the argon gas = ?

V= Volume of the gas = 1.00 L

T= Temperature of the gas = 25°C = 298 K       (0°C = 273 K)

R= Gas constant = 0.0821 atmL/K mol

n=  moles of gas = \frac{\text {given mass}}{\text {Molar mass}}=\frac{1.10g}{40g/mol}=0.0275moles

P=\frac{nRT}{V}=\frac{0.0275\times 0.0821\times 298}{1.00}=0.673atm

Thus the partial pressure of argon is 0.673 atm.

b) According to Dalton's law, the total pressure is the sum of individual pressures.

p_{total}=p_1+p_2

p_{total}=p_{Ar}+p_{ethane}

1.100=0.673+p_{ethane}

1.100-0.673=p_{ethane}

p_{ethane}=0.427atm

Thus partial pressure of ethane is 0.427 atm.

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3 years ago
If u have 10 moles of C2H2 how many mole of O2 would you need
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How does Dr.Hoffmann's ultrasound device benefit society? ( modern chemistry textbook page 180).
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If a sample of sodium chloride with a mass of
alex41 [277]
Original molarity was 1.7 moles of NaCl

Final molarity was 0.36 moles of NaCl

Given Information:

Original (concentrated) solution: 25 g NaCl in a 250 mL solution, solve for molarity

Final (diluted) solution: More water is added to make the new total volume 1.2 liters, solve for the new molarity

1. Solve for the molarity of the original (concentrated) solution.

Molarity (M) = moles of solute (mol) / liters of solution (L)

Convert the given information to the appropriate units before plugging in and solving for molarity.

Molarity (M) = 0.43 mol NaCl solute / 0.250 L solution = 1.7 M NaCl (original solution)

2. Solve for the molarity of the final (diluted) solution.

Remember that the amount of solute remains constant in a dilution problem; it is just the total volume of the solution that changes due to the addition of solvent.

Molarity (M) = 0.43 mol NaCl solute / 1.2 L solution

Molarity (M) of the final solution = 0.36 M NaCl

I hope this helped:))
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