We read your photo as:

How many grams of Na are present in 30 g of NaOH?

Chemistry

ScanSolve AI Answer

Answers

2 parts
1

C. 17 g\text{C. 17 g}

2

D. 101 L\text{D. 101 L}

Step-by-step solution

8 steps

Here are the solutions to the questions:

Part 1· 4 steps

How many grams of Na are present in 30 g of NaOH?

  1. Determine the molar mass of NaOH.

    The atomic mass of Na is 22.99 g/mol22.99 \text{ g/mol}.
    The atomic mass of O is 16.00 g/mol16.00 \text{ g/mol}.
    The atomic mass of H is 1.01 g/mol1.01 \text{ g/mol}.

    Molar mass of NaOH=22.99+16.00+1.01=40.00 g/mol\text{Molar mass of NaOH} = 22.99 + 16.00 + 1.01 = 40.00 \text{ g/mol}

  2. Calculate the number of moles of NaOH in 30 g.

    Moles of NaOH=30 g40.00 g/mol=0.75 mol\text{Moles of NaOH} = \frac{30 \text{ g}}{40.00 \text{ g/mol}} = 0.75 \text{ mol}

  3. Determine the moles of Na in 0.75 mol of NaOH.

    From the chemical formula NaOH, there is 1 mole of Na for every 1 mole of NaOH.
    Therefore, moles of Na = 0.75 mol0.75 \text{ mol}.

  4. Calculate the mass of Na.

    Mass of Na=0.75 mol×22.99 g/mol=17.2425 g\text{Mass of Na} = 0.75 \text{ mol} \times 22.99 \text{ g/mol} = 17.2425 \text{ g}

    The closest option is C.
    The final answer is C. 17 g\boxed{\text{C. 17 g}}.

Part 2

D. 101 L\text{D. 101 L}

How many liters of H2_2 can be produced by the decomposition of 3 moles of NH3_3, at STP?

  1. Write the balanced chemical equation for the decomposition of NH3_3.

    2NH3(g)→N2(g)+3H2(g)2\text{NH}_3(g) \rightarrow \text{N}_2(g) + 3\text{H}_2(g)

  2. Use stoichiometry to find the moles of H2_2 produced from 3 moles of NH3_3.

    From the balanced equation, 2 moles of NH3_3 produce 3 moles of H2_2.

    Moles of H2=3 mol NH3×3 mol H22 mol NH3=4.5 mol H2\text{Moles of H}_2 = 3 \text{ mol NH}_3 \times \frac{3 \text{ mol H}_2}{2 \text{ mol NH}_3} = 4.5 \text{ mol H}_2

  3. Calculate the volume of H2_2 at STP.

    At Standard Temperature and Pressure (STP), 1 mole of any ideal gas occupies 22.4 L22.4 \text{ L}.

    Volume of H2=4.5 mol×22.4 L/mol=100.8 L\text{Volume of H}_2 = 4.5 \text{ mol} \times 22.4 \text{ L/mol} = 100.8 \text{ L}

    The closest option is D.
    The final answer is D. 101 L\boxed{\text{D. 101 L}}.

Part 3· 1 step

If you collected a sample of 3.50 moles of hydrogen gas, H2_2, and heated it in a 10.00 liter container to a temperature of 300K, how much pressure would the H2_2 exert on the container?

  1. Step 1

Was this helpful?

Try one yourself

A new problem that tests the same skill.

Still stuck on this one?

Ask a follow-up, and the answer starts from this question.

Got a different question?Ask your own question

More Chemistry Questions

QWhich of the following questions does the provided solution answer: How many grams of Na are present…QCalculate the moles of sodium hydroxide (NaOH) used.QCalculate the molarity of a 0.5 L solution containing 4 g of NaOH.QCalculate the moles of NaOH used in the titration.QCalculate the pH of the solution after adding 20.0 mL of 0.100 M NaOH to 30.0 mL of 0.100 M HNO₃.
See all Chemistry questions →
Got a syllabus? Photograph it and I'll tell you what's due and what's worth the most.
Handwritten step-by-step solution preview

Handwritten Step-by-Step Solution

Get this as a handwritten image on WhatsApp — like a tutor wrote it for you.

Try on WhatsApp