Calculate the calories of heat required to melt 35.0 g of ice.

A cylinder contains 3.1 L of oxygen at 300 K and 2.7 atm. The gas is heated, causing a piston in the cylinder to move outward. T

zubka84 [21]

Answer: The moles of gas present in the cylinder is 0.34 moles.

Explanation:

Given: $P_{1}$ = 2.7 atm, $V_{1}$ = 3.1 L, $T_{1}$ = 300 K

$P_{2}$ = ?, $V_{2}$ = 9.4 L, $T_{2}$ = 610 K

Formula used to calculate the final temperature is as follows.

$\frac{P_{1}V_{1}}{T_{1}} = \frac{P_{2}V_{2}}{T_{2}}$

Substitute the values into above formula as follows.

$\frac{P_{1}V_{1}}{T_{1}} = \frac{P_{2}V_{2}}{T_{2}}\\\frac{2.7 atm \times 3.1 L}{300 K} = \frac{P_{2} \times 9.4 L}{610 K}\\P_{2} = \frac{5105.7}{2820} atm\\= 1.81 atm$

Now, moles present upon heating the cylinder are as follows.

$P_{2}V_{2} = n_{2}RT_{2}\\1.81 atm \times 9.4 L = n_{2} \times 0.0821 L atm/mol K \times 610 K\\n_{2} = \frac{17.014}{50.081} mol\\= 0.34 mol$

Thus, we can conclude that moles of gas present in the cylinder is 0.34 moles.

6 0

3 years ago

What is the major defining property of gasses?.

jonny [76]

Answer:

Gases have no definite shape or volume. They are fluid, allowing particles/molecules to move freely.

The behavior of a gas is that the volume changes directly with temperature. With a constant volume, the pressure will be directly proportional to the amount of gas.

Explanation:

These are some of the properties I can think of

5 0

2 years ago

The Top Thrill Dragster, a rollercoaster at Cedar Point in Ohio, soars through the air at 176ft/sec. How fast is this in mph?

scoray [572]

Answer:

120mph

Explanation:

Google

divide the speed value by 1.467

or

176 times 60 second in a minute times 60 minutes in an hour

than divide by 5280 the amount of feet in a mile

7 0

3 years ago

Predict the products when cyclohexanol is dehydrated.

lubasha [3.4K]

<span>When cyclohexanol is dehydrated using various means it creates a new hydrocarbon. This new hydrocarbon is called cyclohexene. Cyclohexene is a liquid which has no color, yet has a very strong smell to it. It is used in common industrial processes, but is also considered somewhat unstable due to it's tendency to form peroxides when exposed to light.</span>

5 0

3 years ago

onsider the following reaction: CaCN2 + 3 H2O → CaCO3 + 2 NH3 105.0 g CaCN2 and 78.0 g H2O are reacted. Assuming 100% efficiency

mestny [16]

Answer : The excess reactant is, $H_2O$

The leftover amount of excess reagent is, 7.2 grams.

Solution : Given,

Mass of $CaCN_2$ = 105.0 g

Mass of $H_2O$ = 78.0 g

Molar mass of $CaCN_2$ = 80.11 g/mole

Molar mass of $H_2O$ = 18 g/mole

Molar mass of $CaCO_3$ = 100.09 g/mole

First we have to calculate the moles of $CaCN_2$ and $H_2O$ .

$\text{ Moles of }CaCN_2=\frac{\text{ Mass of }CaCN_2}{\text{ Molar mass of }CaCN_2}=\frac{105.0g}{80.11g/mole}=1.31moles$

$\text{ Moles of }H_2O=\frac{\text{ Mass of }H_2O}{\text{ Molar mass of }H_2O}=\frac{78.0g}{18g/mole}=4.33moles$

Now we have to calculate the limiting and excess reagent.

The balanced chemical reaction is,

$CaCN_2+3H_2O\rightarrow CaCO_3+2NH_3$

From the balanced reaction we conclude that

As, 1 mole of $CaCN_2$ react with 3 mole of $H_2O$

So, 1.31 moles of $CaCN_2$ react with $1.31\times 3=3.93$ moles of $H_2O$

From this we conclude that, $H_2O$ is an excess reagent because the given moles are greater than the required moles and $CaCN_2$ is a limiting reagent and it limits the formation of product.

Left moles of excess reactant = 4.33 - 3.93 = 0.4 moles

Now we have to calculate the mass of excess reactant.

$\text{ Mass of excess reactant}=\text{ Moles of excess reactant}\times \text{ Molar mass of excess reactant}(H_2O)$

$\text{ Mass of excess reactant}=(0.4moles)\times (18g/mole)=7.2g$

Thus, the leftover amount of excess reagent is, 7.2 grams.

8 0

4 years ago