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One cubic meter of an ideal gas at 600 K and 1000 KPa expand to five times its initial volume as follows:(a) By a mechanically reversible, isothermal process [T 2 = 600K; P 2 = 200kPa; W= -1609 kJ]

(b) By a mechanically reversible, adiabatic process [T 2 =208.96K; P 2 = 67.65 kPa; W= -994.4 kJ] For each case calculate the final temperature, pressure and the work done by the gas. C p =21 Jmol- 1K-1.

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Answer 1

Answer:

Answer:

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Explanation:lol just grabbing your points

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100.0 mL of Ca(OH)2 solution is titrated with 5.00 x 10–2 M HBr. It requires 36.5 mL of the acid solution for neutralization. What is the number of moles of HBr used, and the concentration of the Ca(OH)2 solution, respectively?

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The number of moles of HBr and the concentration of the Ca(OH)2 solution is:

The number of moles HBr is = 0.001825

The concentration of Ca(OH)2 is= 0.009125 M

What is the Acid solution for neutralization?

Data given as per question:

The Volume of the Ca(OH)2 is = 100.0 mL = 0.100 L

Then, Molarity of HBr is = 5.00 * 10^-2 M

After that Volume of HBR is = 36.5 mL = 0.0365 L

When The balanced equation is:

Then, Ca(OH)2 + 2HBr → CaBr2 + 2H2O

Then the Calculate molarity of Ca(OH) 2

After that b*Va* Ca is = a * Vb*Cb

Then ⇒with b = the coefficient of HBr is = 2

Now, ⇒with Va = the volume of Ca(OH)2 is = 0.100 L

After that ⇒with ca is = the concentration of Ca(OH)2 = TO BE DETERMINED

Now, ⇒with a = the coefficient of Ca(OH)2 = 1

Then ⇒with Vb is = the volume of HBr = 0.0365 L

Now, ⇒with Cb is = the concentration of HBr = 5.00 * 10^-2 = 0.05 M

Then 2 * 0.100 * Ca = 1 * 0.0365 * 0.05

Now, Ca is = (0.0365*0.05) / 0.200

Therefore, Ca is = 0.009125 M

After that, we Calculate moles HBr

Moles HBr = concentration HBr * volume HBr

Moles HBr = 0.05 M * 0.0365 L

Moles HBr = 0.001825 moles

Find more information Acid solution for neutralization here:

brainly.com/question/203541

Answer:

The number of moles HBr = 0.001825

The concentration of Ca(OH)2 = 0.009125 M

Explanation:

Step 1: Data given

Volume of the Ca(OH)2 = 100.0 mL = 0.100 L

Molarity of HBr = 5.00 * 10^-2 M

Volume of HBR = 36.5 mL = 0.0365 L

Step 2: The balanced equation

Ca(OH)2 + 2HBr → CaBr2 + 2H2O

Step 3: Calculate molarity of Ca(OH) 2

b*Va* Ca = a * Vb*Cb

⇒with b = the coefficient of HBr = 2

⇒with Va = the volume of Ca(OH)2 = 0.100 L

⇒with ca = the concentration of Ca(OH)2 = TO BE DETERMINED

⇒with a = the coefficient of Ca(OH)2 = 1

⇒with Vb = the volume of HBr = 0.0365 L

⇒with Cb = the concentration of HBr = 5.00 * 10^-2 = 0.05 M

2 * 0.100 * Ca = 1 * 0.0365 * 0.05

Ca = (0.0365*0.05) / 0.200

Ca = 0.009125 M

Step 4: Calculate moles HBr

Moles HBr = concentration HBr * volume HBr

Moles HBr = 0.05 M * 0.0365 L

Moles HBr = 0.001825 moles

Hi ! Could someone help me out with this last part to my chemistry practice ? Thank you !

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After 100years, sample is 250g

After 200 years, sample is 125g

After 300years, sample is 62.5 g

Complete combustion of 7.80 g of a hydrocarbon produced 25.1 g of CO2 and 8.55 g of H2O. What is the empirical formula for the hydrocarbon? Insert subscripts as necessary

Answers

Answer:

The empirical formula is C3H5

Explanation:

Step 1: Data given

Mass of the compound = 7.80 grams

Mass of CO2 = 25.1 grams

Molar mass of CO2 = 44.01 g/mol

Mass of H2O = 8.55 grams

Molar mass of H2O = 18.02 g/mol

Molar mass C = 12.01 g/mol

Molar mass H = 1.01 g/mol

Molar mass O = 16.0 g/mol

Step 2: Calculate moles CO2

Moles CO2 = mass CO2 / molar mass CO2

Moles CO2 = 25.1 grams / 44.01 g/mol

Moles CO2 = 0.570 moles

Step 3: Calculate moles C

For 1 mol CO2 we have 1 mol C

For 0.570 moles CO2 we have 0.570 moles C

Step 4: Calculate mass C

Mass C = 0.570 moles * 12.01 g/mol

Mass C = 6.846 grams

Step 5: Calculate moles H2O

Moles H2O = 8.55 grams / 18.02 g/mol

Moles H2O = 0.474 moles

Step 6: Calculate moles H

For 1 mol H2O we have 2 moles H

For 0.474 moles H2O we have 2*0.474 = 0.948 moles H

Step 7: Calculate mass H

Mass H = 0.948 moles * 1.01 g/mol

Mass H = 0.957 grams

Step 8: Calculate mol ratio

We divide by the smallest amount of moles

C: 0.570 moles / 0.570 = 1

H: 0.948 moles / 0.570 = 1.66

This means for 1 mol C we have 1.66 moles H OR for 3 moles C we have 5 moles H

The empirical formula is C3H5

Final answer:

To find the empirical formula of the hydrocarbon, divide the moles of CO2 and H2O by their molar masses. Use the smallest mole ratio to determine the empirical formula.

Explanation:

To find the empirical formula of the hydrocarbon, we need to determine the mole ratios between carbon and hydrogen in the compound. First, calculate the moles of CO2 produced by dividing the mass of CO2 by its molar mass. Next, calculate the moles of H2O produced by dividing the mass of H2O by its molar mass. Finally, divide the moles of each element by the smallest number of moles to obtain the mole ratio between carbon and hydrogen. The empirical formula is CnHm, where n and m represent the mole ratios of carbon and hydrogen, respectively.