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Pavlova-9 [17]
2 years ago
15

Does anybody know how to do this if so please help !

Chemistry
1 answer:
Viktor [21]2 years ago
3 0

Answer:

add x to 7 and divide by 3

Explanation:

easier formula

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A student attempts to separate 4.656 g of a sand/salt mixture just like you did in this lab. After carrying out the experiment,
nikitadnepr [17]

Answer:

Explanation:

a ) Total mixture = 4.656 g

Sand recovered = 2.775 g

percent composition of sand in the mixture

= (2.775 g / 4.656 g ) x 100

= 59.6 % .

b )

Total of sand and salt recovered = 2.775 g + .852 g = 3.627 g .

Total mixture = 4.656 g

percent recovery = (3.627 / 4.656 ) x 100

= 77.9 % .

4 0
3 years ago
Francine makes several measurements of the mass of a metal block. The data set is shown in the table below.
BARSIC [14]

Answer:

Mean

Explanation:

The mean of a series of measurements is calculated when a<em>ll the measurements are added up and then divided by the number of measurements taken</em>, as follows:

  • Sum of Measurements = 20.73 + 20.76 + 20.68 + 20.75 = 82.92

As<u> there are 4 measurements</u>, the mean is:

  • Mean = 82.92 / 4 = 20.73
3 0
3 years ago
Juan Carlos placed 35 grams of ke into a dry, 200-gram container. The top of the container was attached tightly. When the ice wa
lianna [129]
Correct answer is D
8 0
3 years ago
Calculate the number of pounds of CO2CO2 released into the atmosphere when a 22.0 gallon22.0 gallon tank of gasoline is burned i
Gnesinka [82]

Answer:

391.28771 pounds of carbon-dioxide was released into the atmosphere when 22.0 gallon tank of gasoline is burned in an automobile engine.

Explanation:

Density of the gasoline ,d= 0.692 g/mL

Volume of gasoline in an tanks,V = 22.0 gallons = 83,279.02 mL

Let mass of the gasoline be M

Density= \frac{Mass}{Volume}

M = V × d = 83,279.02 mL × 0.692 g/mL=57,629.081 g

Given that gasoline is primarily octane.

2C_8H_{18}+25O_2\rightarrow 16CO_2+18H_2O

Mass of octane burnt in the tank = M = 57,629.081 g

Moles of octane =\frac{57,629.081 g}{114.08g/mol}=505.1637 mol

According to reaction, 2 moles of octane gives 16 moles of carbon-dioxide.

Then 505.1637 mol of octane will give:

\frac{16}{2}\times 505.1637 mol=4,041.3100 mol of carbon-dioxide

Mass of 4,041.3100 mol of carbon-dioxide:

4,041.3100 mol × 44.01 g/mol = 177,858.05 g

Mass of carbon-dioxide produced in pounds = 391.28771 pounds

391.28771 pounds of carbon-dioxide was released into the atmosphere when 22.0 gallon tank of gasoline is burned in an automobile engine.

3 0
3 years ago
What is the pressure of 1.20 moles of SO2 gas in a 4L container at 30 degrees celsius
geniusboy [140]
Let suppose the Gas is acting Ideally, Then According to Ideal Gas Equation,

                                       P V  =  n R T
Solving for P,
                                       P  =  n R T / V     ----- (1)
Data Given;

Moles  = n = 1.20 mol

Volume  = V =  4 L

Temperature  = T = 30 + 273 = 303 K

Gas Constant  = R = 0.08206 atm.L.mol⁻¹.K⁻¹

Putting Values in Eq.1,

                     P  =  (1.20 mol × 0.08206 atm.L.mol⁻¹.K⁻¹ × 303 K) ÷ 4 L

                     P  =  7.45 atm
6 0
3 years ago
Read 2 more answers
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