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4 years ago

Convert 121 points for K PA into TORR

1 answer:

5 0

121 kPa to Torr?

we need a couple of conversions

1 atm = 760 torr
1 atm= 101 kPa

now we use them

121 kPa $\frac{1 atm}{101 kPa}$ x $\frac{760 torr}{1 atm}$ = 910 torr

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Calculate the amount of grams of water that was used when 5525J of energy was used to boil this amount of water.

djverab [1.8K]

Answer:

2.445 g

Explanation:

Step 1: Given and required data

Energy in the form of heat required to boil the water (Q): 5525 J

Latent heat of vaporization of water (∆H°vap): 2260 J/g

Mass of water (m): ?

Step 2: Calculate the mass of water

We will use the following expression.

Q = ∆H°vap × m

m = Q / ∆H°vap

m = 5525 J / (2260 J/g)

m = 2.445 g

4 0

3 years ago

What celsius temperature, t2, is required to change the volume of the gas sample in part a (t1 = 43 ∘c , v1= 1.13×103 l ) to a v

mamaluj [8]

In this case, you are given the temperature and volume of the gas. To answer this question, you will need to use PV=nRT formula. Since the number of molecule and pressure is not changed then you can put 1 in both equations. The formula will become:

PV=nRT
1 V= 1 T
V=T
T/V= 1

Dont forget that the celcius unit should be converted into kelvin. Then the calculation to find the temperature would be:
T1/V1 = T2/V2
(43+273)/ 1.13x10^3 = T2/ 2.26 x 10^3
T2= (2.26 * 10^3) / (1.13 * 10^3) * (43+273)
T2= 2* 316= 632° K= 359°C

6 0

3 years ago

When 10.0 grams of CH4 reacts completely with 40.0 grams of O2 such that there are no reactants left over, 27.5 grams of carbon

BARSIC [14]

Answer:

$\boxed{\text{27.4 g CO$_{2}$; 22.5 g H$_{2}$O}}}$

Explanation:

We know we will need an equation with masses and molar masses, so let’s gather all the information in one place.

M_r: 16.04 32.00 44.01 18.02

CH₄ + 2O₂ → CO₂ + 2H₂O

m/g: 10.0 40.0

1. Moles of CH₄

$\text{Moles of CH}_{4} = \text{10.0 g CH}_{4} \times \dfrac{\text{1 mol CH}_{4}}{\text{16.04 g CH}_{4}} = \text{0.6234 mol CH}_{4}$

2. Mass of CO₂

(i) Calculate the moles of CO₂

The molar ratio is (1 mol CO₂ /1 mol CH₄)

$\text{Moles of CO$_{2}$} = \text{0.6234 mol CH$_4$} \times \dfrac{\text{1 mol CO$_{2}$}} {\text{1 mol CH$_{4}$}} = \text{0.6234 mol CO$_{2}$}$

(ii) Calculate the mass of CO₂

$\text{Mass of CO$_{2}$} = \text{0.6234 mol CO$_{2}$} \times \dfrac{\text{44.01 g CO$_{2}$}}{\text{1 mol CO$_{2}$}} = \textbf{27.4 g CO$_{2}$}\\\\\text{The mass of carbon dioxide formed is } \boxed{\textbf{27.4 g CO$_{2}$}}$

3. Mass of H₂O

(i) Calculate the moles of H₂O

The molar ratio is (2 mol H₂O /1 mol CH₄)

$\text{Moles of H$_{2}$O}= \text{0.6234 mol CH}_{4} \times \dfrac{\text{2 mol H$_{2}$O}}{\text{1 mol CH$_{4}$}} = \text{1.247 mol H$_{2}$O}$

(ii) Calculate the mass of H₂O

$\text{Mass of H$_{2}$O} = \text{1.247 mol H$_{2}$O } \times \dfrac{\text{18.02 g H$_{2}$O}}{\text{1 mol H$_{2}$O}} = \textbf{22.5 g H$_{2}$O}\\\\\text{The mass of water formed is } \boxed{\textbf{22.5 g H$_{2}$O}}$

4 0

3 years ago

Where did coal originate ?<br>

liubo4ka [24]

Answer:

Coal is a fossil fuel and is the altered remains of prehistoric vegetation that originally accumulated in swamps and peat bogs

8 0

4 years ago

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Explain how rocks salt forms in desserts

Fofino [41]

It is typically formed by the evaporation of salty water (such as sea water) which contains dissolved Na+ and Cl- ions. One finds rock salt deposits ringing dry lake beds, inland marginal seas, and enclosed bays and estuaries in arid regions of the world

4 0

3 years ago

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