Which of the following can be true about a chemical reaction

A graduated cylinder is filled with 60.0 ml of water. A cube, made of aluminum, is carefully dropped into the cylinder. Aluminum

katen-ka-za [31]

Answer:

65 ml

Explanation:

The aluminum will not float , so it will displace a volume of fluid equal to its volume.

13.5 gm / 2.7 gm/ml = 5 ml

the new graduated cylinder measurement will be 60 + 5 = 65 ml

3 0

2 years ago

a. If 42.5 g of CH3OH reacts with 22.8 L of O2 at 27°C and a pressure of 2.00 atm, calculate the number of grams of water vapor

Korvikt [17]

Answer:

The mass of water vapor is 44.46 grams

The volume of water is 30.37 L

Explanation:

Step 1: Data given

Mass of CH3OH =42.5 grams

Molar mass CH3OH = 32.04 g/mol

Volume of O2 = 22.8 L

Pressure = 2.00 atm

Step 2: The balanced equation

2CH3OH + 3O2 → 2CO2 + 4H2O

Step 3: Calculate moles CH3OH

Moles CH3OH = mass CH3OH / molar mass CH3OH

Moles CH3OH = 42.5 grams / 32.04 g/mol

Moles CH3OH = 1.326 moles

Step 4: Calculate moles O2

p*V = n*R*T

⇒with p = the pressure = 2.00 atm

⇒with V = the volume of O2 = 22.8 L

⇒with n = the moles of O2 = TO BE DETERMINED

⇒with R = the gas constant = 0.08206 L*Atm/mol*K

⇒with T = the temperature = 27 °C = 300 K

n = (p*V) / (R*T)

n = (2.00 * 22.8) / (0.08206*300)

n = 1.85 moles

Step 5: Calculate the limiting reactant

For 2 moles CH3OH we need 3 moles O2 to produce 2 moles CO2 and 4 H2O

O2 is the limiting reactant. It will completely be consumed ( 1.85 moles). CH3OH is in excess. There will react 2/3*1.85 = 1.233 moles. There will remain 1.326 - 1.233 = 0.093 moles

Step 6: Calculate moles products

For 2 moles CH3OH we need 3 moles O2 to produce 2 moles CO2 and 4 H2O

For 1.85 moles O2 we'll have 1.233 moles CO2 and 2.467 moles H2O

Step 7: Calculate mass H2O

Mass H2O = moles H2O * molar mass H2O

Mass H2O = 2.467 moles * 18.02 g/mol

Mass H2O = 44.46 grams

Step 8: Calculate volume H2O

p*V = n*R*T

⇒with p = the pressure = 2.00 atm

⇒with V = the volume of H2O = TO BE DETERMINED

⇒with n = the moles of H2O = 2.467 moles

⇒with R = the gas constant = 0.08206 L*Atm/mol*K

⇒with T = the temperature = 27 °C = 300 K

V = (n*R*T)/p

V = (2.467 * 0.08206 * 300) / 2.00

V = 30.37 L

The mass of water vapor is 44.46 grams

The volume of water is 30.37 L

3 0

3 years ago

What would be the resulting molarity of a solution made by dissolving 21.9 grams of KCl in enough water to make an 869-millilite

viktelen [127]

Molar mass KCl = <span>74.5513 g/mol

Number of moles:

21.9 / 74.5513 => 0.293 moles

Volume = 869 mL / 1000 => 0.869 L

Molarity = moles / Volume

Molarity = 0.293 / 0.869

=> 0.337 M</span>

8 0

4 years ago

A scientist observes that an unknown solution turns blue Litmus paper red and reacts with zinc to produce hydrogen gas. Which of

Tatiana [17]

The answer is B: an acid

7 0

3 years ago

A reaction between liquid reactants takes place at in a sealed, evacuated vessel with a measured volume of . Measurements show t

Oxana [17]

This question is incomplete, the complete question;

A reaction between liquid reactants takes place at 16°C in a sealed, evacuated vessel with a measured volume of 10.0 L . Measurements show that the reaction produced 37.g of dinitrogen monoxide gas.

Calculate the pressure of dinitrogen monoxide gas in the reaction vessel after the reaction. You may ignore the volume of the liquid reactants. Round your answer to 2 significant digits.

Answer:

Explanation:

Given that;

Volume = 10.0 L

Temperature T = 16°C = ( 16 + 273) = 289 K

we know that molar mass of N₂O = 44 g/mol

number number of moles n will be: weight/molar mass = 37/44 = 0.8409 moles

Universal Gas constant R = 0.0821 atm.mol⁻¹.k⁻¹

pressure p = ?

from the ideal gas law

PV = nRT

P = nRT / n

so we substitute

P = (0.8409 mole × 0.0821 atm.mol⁻¹.k⁻¹ × 289 K) / 10.0 l

P = 19.95195 / 10.0

P = 1.9952 atm

6 0

3 years ago