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KATRIN_1 [288]
3 years ago
13

Dustin is mixing concrete. A formula for concrete calls for 3/8 gal of water. Dustin wants to make 7/9 more concrete than the fo

rmula creates. How much water should Dustin use?Simplify your answer.
Chemistry
1 answer:
slava [35]3 years ago
5 0
We can use a ratio to solve this question. Lets refer to the amount formed by the formula as a serving
1 serving needs 3/8 gal
We want to create 7/9 servings extra, so
1 + 7/9 = 16/7
1 : 3/8
16/7 : x
1/(3/8) = (16/7) / x
8 / 3 = 16x / 7
x = 7/6
He needs to use 7/6 gallons of water.
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GalinKa [24]

Answer:

Solar eclipse

Explanation:

A solar eclipse occurs when a portion of the Earth is engulfed in a shadow cast by the Moon which fully or partially blocks sunlight. This occurs when the Sun, Moon and Earth are aligned. Such alignment coincides with a new moon indicating the Moon

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2 years ago
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Question<br> What is the name of the covalent compound with the formula P2N3?
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2 years ago
The volume of an automobile air bag was 66.8 L when inflated at 25 °C with 77.8 g of nitrogen gas. What was the pressure in the
Ray Of Light [21]

Answer:

\large \boxed{\text{103 kPa}}

Explanation:

We can use the Ideal Gas Law — pV = nRT

Data:

V = 66.8 L

m = 77.8 g

T = 25 °C

Calculations:

(a) Moles of N₂

\text{Moles of N}_{2} = \text{77.8 g N}_{2} \times \dfrac{\text{1 mol N}_{2}}{\text{28.01 g N}_{2}} = \text{2.778 mol N}_{2}

(b) Convert the temperature to kelvins

T = (25 + 273.15) K = 298.15 K

(c) Calculate the pressure

\begin{array}{rcl}pV & =& nRT\\p \times \text{66.8 L} & = & \text{2.778 mol} \times \text{8.314 kPa$\cdot$ L$\cdot$K$^{-1}$mol$^{-1}\times$ 298.15 K}\\66.8p & = & \text{6886 kPa}\\p & = & \textbf{103 kPa}\end{array}\\\text{The pressure in the bag is $\large \boxed{\textbf{103 kPa}}$}

3 0
2 years ago
Today is Earth day. What is one thing that you can do at school or at home to help protect our home, planet Earth?
omeli [17]
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7 0
2 years ago
A 21.8 g sample of ethanol (C2H5OH) is burned in a bomb calorimeter, according to the following reaction. If the temperature ris
Blababa [14]

<u>Answer:</u> The heat capacity of calorimeter is 15.66J/^oC

<u>Explanation:</u>

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

\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}

Given mass of ethanol = 21.8 g

Molar mass of ethanol = 46.07 g/mol

Putting values in above equation, we get:

\text{Moles of ethanol}=\frac{21.8g}{46.07g/mol}=0.473mol

To calculate the enthalpy change of the reaction, we use the equation:

\Delta H_{rxn}=\frac{q}{n}

where,

q = amount of heat released = ?

n = number of moles = 0.473 moles

\Delta H_{rxn} = enthalpy change of the reaction  = -1235 kJ/mol = -1235\times 10^3J/mol     (Conversion factor:  1 kJ = 1000 J)

Putting values in above equation, we get:

-1235\times 10^3J/mol=\frac{q}{0.473mol}\\\\q=(-1235\times 10^3J/mol\times 0.473mol)=-584.16\times 10^3J

To calculate the heat capacity of calorimeter, we use the equation:

q=c\Delta T

where,

q = heat absorbed by the calorimeter = 584.16\times 10^3J

c = heat capacity = ?

\Delta T = change in temperature = T_2-T_1=62.3^oC-25^oC=37.3^oC

Putting values in above equation, we get:

584.16\times 10^3J=c\times 37.3^oC\\\\c=\frac{584.16\times 10^3J}{37.3^oC}=15.66J/^oC

Hence, the heat capacity of calorimeter is 15.66J/^oC

4 0
3 years ago
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