At absolute zero, the average kinetic energy of the molecules is zero. True False

Bromine occurs in the ____ state at room temperature.

Studentka2010 [4]

Answer:

d liquid

Explanation:

Bromine occurs in the liquid state at room temperature.

Bromine is the only nonmetallic element that occurs in the liquid state at room temperature.

6 0

3 years ago

How many grams of water are produced from the combustion of 45.2 g of

Zina [86]

Answer:

101.56 of H₂O

Explanation:

The balanced equation for the reaction is given below:

CH₄ + 2O₂ —> CO₂ + 2H₂O

Next, we shall determine the mass of CH₄ that reacted and the mass of H₂O produced from the balanced equation. This is illustrated below:

Molar mass of CH₄ = 12 + (4×1.01)

= 12 + 4.04

= 16.04 g/mol

Mass of CH₄ from the balanced equation = 1 × 16.04 = 16.04 g

Molar mass of H₂O = (2×1.01) + 16

= 2.02 + 16

= 18.02 g/mol

Mass of H₂O from the balanced equation = 2 × 18.02 = 36.04g

SUMMARY:

From the balanced equation above,

16.04 g of CH₄ reacted to produce 36.04 g of H₂O.

Finally, we shall determine the mass of water, H₂O produced by the reaction of 45.2 g of methane, CH₄. This can be obtained as illustrated below:

From the balanced equation above,

16.04 g of CH₄ reacted to produce 36.04 g of H₂O.

Therefore 45.2 g of CH₄ will react to produce = (45.2 × 36.04)/16.04 = 101.56 g of H₂O.

Thus, 101.56 of H₂O were obtained.

7 0

3 years ago

What is another name for a Grasshopper?

Alchen [17]

Answer:

The scientific name of the grasshopper is Caelifera.

Explanation:

hope this helps.

3 0

3 years ago

Read 2 more answers

Identify which of the following oxidation-reduction reactions are balanced and which are unbalanced in both mass and charge. 1.2

Ivenika [448]

Answer:

1. Balanced

2. Unbalanced

3. Unbalanced

Explanation:

Identify which of the following oxidation-reduction reactions are balanced and which are unbalanced in both mass and charge.

1. Ag⁺(aq) + Li(s) → Ag(s) + Li⁺(aq)

This reaction is balanced in both mass and charge.

2. Fe(s) + Na⁺(aq) → Fe²⁺(aq) + Na(s)

This reaction is balanced in mass but unbalanced in charge since the charge to the left is +1 and the charge to the right is 2+.

3. K(s) + H₂O(l) → KOH(aq) + H₂(g)

This reaction is balanced in charge but unbalanced in mass since there are 2 atoms of H to the left and 3 atoms of H to the right.

3 0

3 years ago

For the following reaction, 5.61 grams of carbon monoxide are mixed with excess water . Assume that the percent yield of carbon

stealth61 [152]

Answer: The ideal yield of carbon dioxide is 7.506 grams

Explanation:

To calculate the number of moles, we use the equation:

$\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}$ .....(1)

Given mass of carbon monoxide = 5.61 g

Molar mass of carbon monoxide = 28 g/mol

Putting values in equation 1, we get:

$\text{Moles of carbon monoxide}=\frac{5.61g}{28g/mol}=0.200mol$

The chemical equation for the reaction of carbon monoxide and water follows:

$CO(g)+H_2O(l)\rightarrow CO_2(g)+H_2(g)$

By Stoichiometry of the reaction:

1 mole of carbon monoxide produces 1 mole of carbon dioxide

So, 0.200 moles of carbon monoxide will produce = $\frac{1}{1}\times 0.200=0.200mol$ of carbon dioxide

Now, calculating the mass of carbon dioxide from equation 1, we get:

Molar mass of carbon dioxide = 44 g/mol

Moles of carbon dioxide = 0.200 moles

Putting values in equation 1, we get:

$0.200mol=\frac{\text{Mass of carbon dioxide}}{44g/mol}\\\\\text{Mass of carbon dioxide}=(0.200mol\times 44g/mol)=8.8g$

To calculate the experimental yield of carbon dioxide, we use the equation:

$\%\text{ yield}=\frac{\text{Experimental yield}}{\text{Theoretical yield}}\times 100$

Percentage yield of carbon dioxide = 85.3 %

Theoretical yield of carbon dioxide = 8.8 g

Putting values in above equation, we get:

$85.3=\frac{\text{Experimental yield of carbon dioxide}}{8.8g}\times 100\\\\\text{Experimental yield of carbon dioxide}=\frac{85.3\times 8.8}{100}=7.506g$

Hence, the ideal yield of carbon dioxide is 7.506 grams

3 0

3 years ago