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3 years ago

CH4(g) + 2O2(g) = CO2(g) + 2H2O(g)

Chemistry

1 answer:

krek1111 [17]3 years ago

3 0

Answer:

0.04 moles of CH₄ are required

Explanation:

Given data:

Number of moles of CH₄ required = ?

Number of moles of O₂ present = 0.08 mol

Solution:

Chemical equation:

CH₄ + 2O₂ → CO₂ + 2H₂O

now we will compare the moles of oxygen and methane.

O₂ : CH₄

2 : 1

0.08 : 1/2×0.08 = 0.04

Thus, 0.04 moles of CH₄ are required.

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Convert 1.45 × 1024 atoms of carbon to moles of carbon.

anygoal [31]

1 mol = 6.02 * 10^23 atoms of carbon
x mol = 1.45 * 10^24 atoms of carbon

1/x =6.02*10^23 / 1.45 * 10^24

6.02 * 10^23 x = 1.45 * 10^24
x = 1.45 * 10^24 / 6.02 * 10^23
x = 2.41 mols of carbon

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3 years ago

#1. Which one of the following statements correctly defines active site? The active site is a site on the enzyme molecule where

deff fn [24]

Active sites in enzymes are where substrates bind. Once they bind, a catalytic reaction occurs as a complex between substrate and enzyme is formed. Enzymes are termed as biocatalysts or simply catalysts since they speed up the catalytic reaction. After the reaction, they simply revert back to their original form, after having adjusted to fit with substrate.

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3 years ago

Analyze complete and balance the following equation co2(g)+hcl(aq)

Anna007 [38]

Answer:

$CO_{2} (g)+4HCl(aq)->2H_{2} O(g)+CCl_{4} (g)$

This is a double displacement reaction, C goes with Cl in the products side and O2 goes with H. All that is left is to balance the equation, making sure each side has equal amounts of atoms.

4 0

2 years ago

Material property of glass

iren2701 [21]

The main characteristics of glass are transparency, heat resistance, pressure, and breakage resistance, and chemical resistance.

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3 years ago

Assuming an efficiency of 30.80%, calculate the actual yield of magnesium nitrate formed from 147.4g of magnesium and excess cop

Reil [10]

Answer:

The answer to your question is 280 g of Mg(NO₃)₂

Explanation:

Data

Efficiency = 30.80 %

Mg(NO₃)₂ = ?

Magnesium = 147.4 g

Copper (II) nitrate = excess

Balanced Reaction

Mg + Cu(NO₃)₂ ⇒ Mg(NO₃)₂ + Cu

Reactants Elements Products

1 Mg 1

1 Cu 1

2 N 2

6 O 6

Process

1.- Calculate the theoretical yield

Molecular weight Mg = 24

Molecular weight Mg(NO₃)₂ = 24 + (14 x 2) + (16 x 6)

= 24 + 28 + 96

= 148 g

24 g of Mg -------------------- 148 g of Mg(NO₃)₂

147.4 g of Mg ------------------- x

x = (147.4 x 148) / 24

x = 908.96 g of Mg(NO₃)₂

2.- Calculate the Actual yield

yield percent = $\frac{actual yield}{theoretical yield}$

Solve for actual yield

Actual yield = Yield percent x Theoretical yield

Substitution

Actual yield = $\frac{30.8}{100}$ x 908.96

Actual yield = 279.95 ≈ 280g

4 0

3 years ago