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3 years ago

7

3. If a gas exerts 1.2 atm of pressure at a volume of 31 liters and a temperature of 360K, how many moles of the gas are in the

container.

1 answer:

Mashcka [7]3 years ago

5 0

The answer is 1.26 Mol

n = PV/RT= (1.2 atm)(31 L) / (0.0821 )(360K) = 1.26 mol H2

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If the density of a 45.0 cm3 block of wood is 0.65 g/ml what is the mass of the wood?

wlad13 [49]

Answer:

$\boxed {\tt mass=29.25 \ grams}$

Explanation:

The density formula is mass over volume.

$d=\frac{m}{v}$

Rearrange the formula for the mass, m. Multiply both sides of the formula by v.

$d*v=\frac{m}{v}*v$

$d*v=m$

Mass can be found by multiplying the density and volume. The density is 0.65 grams per milliliter and the volume is 45.0 cubic centimeters.

A cubic centimeter is equal to a milliliter.

Therefore, 45 cubic centimeters also equals 45 milliliters.

$d= 0.65 \ g/mL\\v= 45 \ mL$

Substitute the values into the formula.

$0.65 \ g/mL * 45 \ mL=m$

Multiply. Note the milliliters, or mL will cancel out.

$0.65 \ g * 45=m$

$29.25 \ g=m$

The mass of the wood is 29.25 grams.

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Explain what happens when an atom gains or looses an electron

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When an atom gains an electron it becomes a negatively charged ion. When an atom looses an electron it becomes positively charged because the number of positively charged protons.

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Based on the article "Will the real atomic model please stand up?,” describe what Dalton’s theory states about a molecule of wat

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When 0.243 g of Mg metal is combined with enough HCl to make 100 mL of solution in a constant-pressure calorimeter, the followin

satela [25.4K]

Answer:

ΔH = - 464 kJ/mol

Explanation:

Step 1: Data given

Mass of Mg = 0.243 grams

volume of solution = 100 mL

Initial temperature = 23.0 °C

Final temperature = 34.1 °C

Specific heat = 4.18 J/g°C

Step 2: Calculate the heat transfer

Q= m*c*ΔT

⇒ m = the mass of the solution = 100 grams

⇒ c = the specific heat of the solution = 4.18 J/g°C

⇒ ΔT = The change in temperature = T2 - T1 = 34.1 - 23.0 = 11.1 °C

Q = 100 g * 4.18 J/g°C * 11.1°C

Q = 4639.8 J

Step 3: Calculate moles of Mg

Moles Mg = 0.243 grams / 24.3 g/mol

Moles Mg = 0.01 moles

Step 4: Calculate ΔH

ΔH = 4639.8 J / 0.01 moles

ΔH = 463980 J/mol = 464 kJ/mol

(4.6398 kJ) / (0.0099979 mol) = 464 kJ/mol

Since the reaction is exothermic, the ΔH is negative by convention, so:

ΔH = - 464 kJ/mol

6 0

3 years ago