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enyata [817]
3 years ago
10

21<2x+3 help fast please ​

Chemistry
2 answers:
kolezko [41]3 years ago
7 0

Answer:

Explanation:

x in (-oo:+oo)

2 < (1/2)*x-3 // - (1/2)*x-3

2-((1/2)*x)+3 < 0

(-1/2)*x+2+3 < 0

5-1/2*x < 0 // - 5

-1/2*x < -5 // : -1/2

x > -5/(-1/2)

x > 10

x in (10:+oo)

(10:+oo)

ValentinkaMS [17]3 years ago
5 0

Answer:

x > 9

Explanation:

21 < 2x + 3

Subtract 3 from both side

21 —3 < 2x + 3 —3

18 < 2x

Divide both side by the coefficient of x i.e 2

18/2 < x

9 < x

Since 9 is less than x, it therefore means that x is grater that 9.

x > 9

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an engineering team is conducting a trial launch of a few rocket . which part is the engineering process is the team in ?
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Answer:

Evaluate the result (Apex)

Explanation:

7 0
3 years ago
What is the volume of one mole of any gas at STP?
Vikki [24]
The volume of one mole of any gas at Standard Temperature and Pressure (1 atm and 0 degrees Celsius [273K]) is 22.4 L.
7 0
3 years ago
A 256 mL sample of HCl gas is in a flask where it exerts a force (pressure) of 67.5 mmHg. What is the pressure of the gas if it
Effectus [21]

Answer:

The pressure in the new flask would be 128\; \rm mmHg if the \rm HCl here acts like an ideal gas.  

Explanation:

Assume that the \rm HCl sample here acts like an ideal gas. By Boyle's Law, the pressure P of the gas should be inversely proportional to its volume V.

For example, let the initial volume and pressure of the sample be V_1 and P_1. The new volume V_2 and pressure P_2 of this sample shall satisfy the equation: P_1 \cdot V_1 =P_2 \cdot V_2.

In this question,

  • The initial volume of the gas is V_1= 256\; \rm mL.
  • The initial pressure of the gas is P_1 = 67.5\; \rm mmHg.
  • The new volume of the gas is V_2 = 135\; \rm mL.

The goal is to find the new pressure of this gas, P_2.

Assume that this sample is indeed an ideal gas. Then the equation P_1 \cdot V_1 =P_2 \cdot V_2 should still hold. Rearrange the equation to separate the unknown, P_2. Note: make sure that the units for V_1 and V_2 are the same before evaluating. That way, the unit of

\begin{aligned} & P_2\\ &= \frac{P_1 \cdot V_1}{V_2} \\ &= \frac{256\; \rm mL \times 67.5\; \rm mmHg}{135\; \rm mL} \\ & \approx 128\; \rm mmHg\end{aligned}.

3 0
3 years ago
Ammonia gas will react with oxygen gas to yield nitrogen monoxide gas and water vapor.
ruslelena [56]

Answer:

a) <u>0.168 moles O2</u>

<u>b) </u> <u>9.50 grams O2</u>

<u>c) 0.01662 kg NO</u>

<u>d)</u>88.9 %

Explanation:

Step 1: Data given

Molar mass of NH3 = 17.03 g/mol

Molar mass of O2 = 32 g/mol

Molar mass of NO = 30.01 g/mol

Molar mass of H2O = 18.02 g/mol

Step 2: The balanced equation:

4NH3 + 5O2 → 4NO + 6H2O

a. How many moles of ammonia will react with 6.73g of oxygen?

Calculate moles of oxygen = mass O2/ molar mass O2

moles oxygen =  6.73 grams / 32.00 g/mol = 0.210 moles

Calculate moles of NH3

For 4 moles of NH3 we need 5 moles O2 to produce 4 moles NO and 6 moles H2O

For 0.210 moles O2 we need 4/5 *0.210 = <u>0.168 moles O2</u>

<u />

b. If 6.42g of water is produced, how many grams of oxygen gas reacted?

Calculate moles of H2O = 6.42 grams / 18.02 g/mol = 0.356 moles

Calculate moles of O2:

For 4 moles of NH3 we need 5 moles O2 to produce 4 moles NO and 6 moles H2O

For 0.356 moles H2O we'll need 5/6 * 0.356 = 0.297 moles O2

Calculate mass of O2 = moles O2 * molar mass O2

Mass O2 = 0.297 moles O2 * 32.00 g/mol =  <u>9.50 grams O2</u>

c. If the reaction uses up 9.43105 g of ammonia, how many kilograms of nitrogen monoxide will be formed?

Calculate moles of ammonia = 9.43105 grams / 17.03 g/mol =0.5538 moles

Calculate moles of NO:

For 4 moles of NH3 we need 5 moles O2 to produce 4 moles NO and 6 moles H2O

For 0.5538 moles of NH3 we'll have 0.5538 moles NO

Calculate mass of NO

Mass NO = 0.5538 moles * 30.01 g/mol = 16.62 grams = <u>0.01662 kg NO</u>

<u />

<u />

d. When 2.51 g of ammonia react with 3.76 g of oxygen, 2.27 g of water vapor are produced. What is the percentage yield of water?

<em>Calculate moles of NH3</em> = 2.51 grams / 17.03 g/mol = 0.147 moles

<em>Calculate moles of O2 </em>= 3.76 grams / 32 g/mol = 0.118 moles

<em>Determine the limiting reactant</em>

O2 is the limiting reactant, it will completely be consumed (0.118 moles)

NH3 is in excess. There will react 4/5 * 0.118 = 0.0944 moles

There will remain 0.147 - 0.0944 = 0.0526 moles

<em>Calculate moles H2O</em>: For 0.118 moles O2 we'll have 6/5 * 0.118 = 0.1416 moles H2O

<em>Calculate mass H2O</em> = 0.1416 moles * 18.02 g/mol = 2.552 grams H2O

<em>Calculate % yield</em> = (2.27/2.552)*100 % = <u>88.9 %</u>

4 0
2 years ago
Which of the following is an example of an experimental scientific investigation
sleet_krkn [62]

Scientific investigation is the process in which scientist solve the problems by using different systematic approach. It can be initiated in different ways.

Experimental Scientific investigation: The investigation in which scientist answer the question on the basis of experimental results. Experimental investigation contains both dependent and independent variables, and only one variable is tested at a time is possible. This process makes uses of collecting observation and identifying the process in physical word.

Noting the colour of a solution when heated is the experimental scientific investigation

Therefore, other given options are part of scientific observation whereas Noting the colour of a solution when heated explains the experimental scientific investigation.



7 0
3 years ago
Read 2 more answers
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