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3 years ago

At a certain temperature and pressure, one liter of CO2 gas weighs 1.95 g.

Chemistry

1 answer:

AysviL [449]3 years ago

7 0

Answer:

1.332 g.

Explanation:

We can use the general law of ideal gas: PV = nRT.

where, P is the pressure of the gas in atm.

V is the volume of the gas in L.

n is the no. of moles of the gas in mol.

R is the general gas constant,

T is the temperature of the gas in K.

At the same T and P and constant V (1.0 L), different gases have the same no. of moles (n):

∴ (n) of CO₂ = (n) of C₂H₆

∵ n = mass/molar mass

∴ (mass/molar mass) of CO₂ = (mass/molar mass) of C₂H₆

mass of CO₂ = 1.95 g, molar mass of CO₂ = 44.01 g/mol.

mass of C₂H₆ = ??? g, molar mass of C₂H₆ = 30.07 g/mol.

∴ mass of C₂H₆ = [(mass/molar mass) of CO₂]*(molar mass) of C₂H₆ = [(1.95 g / 44.01 g/mol)] * (30.07 g/mol) = 1.332 g.

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When a 0.245-g sample of benzoic acid is combusted in a bomb calorimeter, the temperature rises 1.643 ∘C . When a 0.260-g sample

sveticcg [70]

Answer:

The heat of combustion per moles of caffeine is 4220 kJ/mol

Explanation:

Step 1: Data given

⇒ When benzoic acid sample of 0.245 grams is burned the temperature rise is 1.643 °C

⇒ When 0.260 gram of caffeine is burned, the temperature rise is 1.436 °C

⇒ Heat of combustion of benzoic acid = 26.38 kJ/g

Step 2: Calculate the heat released: for combustion of benzoic acid

0.245 g benzoic acid * 26.38 kJ/g = 6.4631 kJ

Step 3: Calculate the heat capacity of the calorimeter:

c = Q/ΔT

Q = 6.4631 kJ / 1.643°C = 3.934 kJ/ °C

Step 4: Calculate moles of a 0.260 g sample of caffeine:

Moles caffeine = Mass caffeine / Molar mass caffeine

0.260 grams/ 194.19 g/mol = 0.0013389 moles

Step 5: Calculate heat released: for combustion of caffeine

Q = c * ΔT

Q = 3.934 kJ/°C * 1.436 °C = 5.65 kJ

Step 6: Calculate the heat of combustion per mole of caffeine

5.65 kJ / 0.0013389 moles = 4219.9 kJ/mol ≈ 4220 kJ/mol

The heat of combustion per moles of caffeine is 4220 kJ/mol

4 0

3 years ago

There are two isotopes of chlorine. below is a list of each and their mass and abundance. calculate the atomic mass of chlorine.

Vesna [10]

Chlorine is very lequid structure

6 0

3 years ago

Which of these elements has an atom with the most stable outer electron configuration? * Cl Ca Ne Na

SashulF [63]

Answer:

Neon (Ne) has the most stable outer electron configuration because the outer electron is completely filled and it has octet structure

Explanation:

The configuration of these elements is as follows;

Cl₁₇ = 2, 8,7 (the outer electron is 7)

Ca₂₀ = 2,8,8,2 (the outer electron is 2)

Ne₁₀ = 2,8 (the outer electron is 8)

Na₁₁ = 2,8,1 (the outer electron is 1)

Based on the outer electron value above, Neon (Ne) has the most stable outer electron configuration because the outer electron is completely filled and it has octet structure.

6 0

3 years ago

A urine sample has a mass of 147 g and a density of 1.020 g/mL. What is the volume of this sample?

son4ous [18]

So we know that the equation for density is:

$D=\frac{m}{V}$

where D is the density, m is the mass in grams, and V is the volume in mL.

So since we know two of the variables, mass and density, we can solve for the volume:

$\frac{1.020g}{mL}=\frac{147g}{V}$

$V=\frac{147g}{\frac{1.020g}{mL}}$

$V=144.12mL$

Therefore, the volume of this urine sample is 144.12mL.

5 0

3 years ago

How many total atoms are in 0.680 g of P₂O5?

Ludmilka [50]

Answer: 2.88× $10^{24}$ atoms $P_{2}O_{5}$

Explanation: First, using stoichiometry, we must convert this from grams to moles, then from moles to atoms.

1. For the first step, we should also look at the periodic table to find the molar mass of the compound, then use that as the denominator.

$0.680g P_{2} O_{5} *\frac{1molP_{2} O_{5} }{141.948gP_{2} O_{5} } =4.79mol P_{2} O_{5}$

2. Now that it is converted to moles, we must convert it to atoms by multiplying it by Avogadro's number.

$4.79molP_{2} O_{5} *\frac{6.022X10^{23} }{1mol} =2.88*10^{24}$

With this information, we know that there are $2.88X10^{24}$ total atoms in 0.680 grams $P_{2} O_{5}$ .

I hope this helps! Pls give brainliest!! :)

8 0

2 years ago