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3 years ago

Calculate the number of grams of oxygen required to convert 48.0 g of glucose to co2 and h2o.

Chemistry

1 answer:

worty [1.4K]3 years ago

4 0

I believe that the balanced chemical reaction is:

C6H12O6 + 6 O2 → 6 CO2 + 6 H2O

So the number of grams of oxygen required is:

mass O2 required = 48 g C6H12O6 * (1 mole C6H12O6 / 180.16 g) * (6 mole O2 / 1 mole C6H12O6) * (32 grams O2 / 1 mole)

mass O2 required = 51.15 grams

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Diatomic iodine [I2] decomposes at high temperature to form I atoms according to the reaction I2(g)⇌2I(g), Kc = 0.011 at 1200∘C

umka2103 [35]

Answer:

The concentration of I at equilibrium = 3.3166×10⁻² M

Explanation:

For the equilibrium reaction,

I₂ (g) ⇄ 2I (g)

The expression for Kc for the reaction is:

$K_c=\frac {\left[I_{Equilibrium} \right]^2}{\left[I_2_{Equilibrium} \right]}$

Given:

$\left[I_2_{Equilibrium} \right]$ = 0.10 M

Kc = 0.011

Applying in the above formula to find the equilibrium concentration of I as:

$0.011=\frac {\left[I_{Equilibrium} \right]^2}{0.10}$

So,

$\left[I_{Equilibrium} \right]^2=0.011\times 0.10$

$\left[I_{Equilibrium} \right]^2=0.0011$

$\left[I_{Equilibrium} \right]=3.3166\times 10^{-2}\ M$

Thus, The concentration of I at equilibrium = 3.3166×10⁻² M

3 0

3 years ago

9.8 x 10^-6 regular notation

topjm [15]

Answer:

0.0000098 should be the answer

Explanation:

3 0

3 years ago

A/An ______ bond occurs when 2 atoms share electrons.

allsm [11]

Answer:

convalent???????

Explanation:

sowwy if it wrong

8 0

2 years ago

a sample of 3.00 g of so2 (g)originally in a 5.00 L vesselat 21 degee Celsius is transferred to a 10.0 L vessel at 26 degree Cel

eimsori [14]

Answer:

1) The partial pressure of SO₂ gas in the larger container = 0.115 atm.

2) The partial pressure of N₂ gas in the larger container = 0.206 atm.

3) The total pressure in the vessel = 0.321 atm.

Explanation:

To calculate the partial pressure of each gas, we can use the general law of ideal gas: PV = nRT.

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

V is the volume of the vessel in L,

n is the no. of moles of the gas,

R is the general gas constant (R = 0.082 L.atm/mol.K),

T is the temperature of the gas in K.

1) What is the partial pressure of SO₂ gas in the larger container?

∵ P = nRT/V.

n = mass/molar mass = (3.0 g)/(64.066 g/mol) = 0.047 mol.

R = 0.082 L.atm/mol.K.

T = 26 °C + 273.15 = 299.15 K.

V = 10.0 L. (The volume of the new container)

∴ P = nRT/V = (0.047 mol)(0.082 L.atm/mol.K)(299.15 K)/(10.0 L) = 0.115 atm.

2) What is the partial pressure of N₂ gas in the larger container?

∵ P = nRT/V.

n = mass/molar mass = (2.35 g)/(28.0 g/mol) = 0.084 mol.

R = 0.082 L.atm/mol.K.

T = 26 °C + 273.15 = 299.15 K.

V = 10.0 L. (The volume of the new container)

∴ P = nRT/V = (0.084 mol)(0.082 L.atm/mol.K)(299.15 K)/(10.0 L) = 0.206 atm.

3) What is the total pressure in the vessel?

According to Dalton's law the total pressure exerted is equal to the sum of the partial pressures of the individual gases.

∵ The total pressure in the vessel = the partial pressure of SO₂ + the partial pressure of N₂.

∴ The total pressure in the vessel = 0.115 + 0.206 = 0.321 atm.

5 0

2 years ago

A compound is 44.7% P and the rest O. Determine its emperical formula.

svet-max [94.6K]

Answer:

P₅O₁₂

Explanation:

Assume that you have 100 g of the compound.

Then you have 44.7 g P and 55.3 g O.

1. Calculate the moles of each atom

Moles of P = 44.7 × 1/30.97 = 1.443 mol Al

Moles of O = 55.3 × 1/16.00 = 3.456 mol O

2. Calculate the molar ratios.

P: 1.443/1.443 = 1

O: 3.456/1.443 = 2.395

3. Multiply by a number to make the ratio close to an integer

P: 5 × 1 = 5

O: 5 × 2.395 = 11.97

3. Determine the empirical formula

Round off all numbers to the closest integer.

P: 5

O: 12

The empirical formula is P₅O₁₂.

6 0

3 years ago