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Nostrana [21]
1 year ago
10

A nurse practitioner prepares an injection of promethazine, an antihistamine used to treat allergic rhinitis. If the stock bottl

e is labeled 30. mg/mL and the order is a dose of 15.0 mg , how many milliliters will the nurse draw up in the syringe?
Chemistry
1 answer:
nordsb [41]1 year ago
5 0
Essentially what the question is asking you to find is the volume of promethazine the nurse will fill the syringe with.  The question gives you :
-  Density =  30 mg / mL
-  Mass    =  15.0 mg

Therefore you can solve using the formula:
    Volume  =   \frac{mass}{density}
                   =   \frac{15 mg}{30 mg / L}
                   =    0.5 mL
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For nitrogen gas the values of Cv and Cp at 25°C are 20.8 J K−1 mol−1 and 29.1 J K−1 mol−1, respectively. When a sample of nitro
kifflom [539]

Answer:

The fraction of energy used to  increase the internal energy of the gas is 0.715

Explanation:

Step 1: Data given

Cv for nitrogen gas = 20.8 J/K*mol

Cp for nitrogen gas = 29.1 J/K*mol

Step 2:

At a constant volume, all the  heat will increase the internal energy of the gas.

At constant pressure, the gas expands and does work., if the volume changes.

Cp= Cv + R

⇒The value needed to change the internal energy is shown by Cv

⇒The work is given by Cp

To find what fraction of the energy is used to increase the internal energy of the gas, we have to calculate the value of Cv/Cp

Cv/Cp = 20.8 J/K*mol / 29.1 J/K*mol

Cv/Cp = 0.715

The fraction of energy used to  increase the internal energy of the gas is 0.715

3 0
1 year ago
Read 2 more answers
Match each situation below to a letter on the illustration.
Mnenie [13.5K]

Answer:a

Explanation:

4 0
1 year ago
When 64.0 g of methanol (CHOH) is burned, 1454 kJ of energy is produced. What is the heat of combustion for methanol?
andreev551 [17]

 The heat  of combustion  for  methanol   is 727  kj/mol


    <em><u>calculation</u></em>

 calculate the moles  of methanol (CH3OH)

moles = mass/molar  mass

molar mass of methanol =  12 +( 1 x3)  +16 + 1= 32 g /mol

moles is therefore= 64.0 g / 32 g/mol =  2 moles


Heat of combustion  is therefore = 1454 Kj / 2 moles =  727  Kj/mol

6 0
1 year ago
How many Ca2+ ions are in a sample of CaSO4 having a total mass of 68.07 g?
harkovskaia [24]

Answer:

There are  

17.01

Explanation:

The chemical formula for calcium phosphate is  

Ca

3

(PO

4

)

2

. This means that in one mole of calcium phosphate, there are three calcium ions and two phosphate ions.

6 0
1 year ago
Consider the chemical reaction: N2 3H2 yields 2NH3. If the concentration of the reactant H2 was increased from 1.0 x 10-2 M to 2
Brilliant_brown [7]

The equilibrium constant of a reaction is defined as:

"The ratio between equilibrium concentrations of products powered to their reaction quotient and  equilibrium concentration of reactants powered to thier reaction quotient".

The reaction quotient, Q, has the same algebraic expressions but use the actual concentrations of reactants.

To solve this question we need this additional information:

<em>For this reaction, K = 6.0x10⁻² and the initial concentrations of the reactants are:</em>

<em>[N₂] = 4.0M; [NH₃] = 1.0x10⁻⁴M and [H₂] = 1.0x10⁻²M</em>

<em />

Thus, for the reaction:

N₂ + 3H₂ ⇄ 2NH₃

The equilibrium constant, K, of this reaction, is defined as:

K = 6.0x10^{-2} = \frac{[NH_3]^2}{[N_2][H_2]^3}

And Q, is:

Q = \frac{[NH_3]^2}{[N_2][H_2]^3}

Where actual concentrations are:

[NH₃] = 1.0x10⁻⁴M

[N₂] = 4.0M

[H₂] = 2.5x10⁻¹M

Replacing:

Q = \frac{[1.0x10^{-4}]^2}{[4.0][2.5x10^{-1}]^3}

<h3>Q = 1.6x10⁻⁷</h3>

As Q < K,

<h3>The chemical system will shift to the right in order to produce more NH₃</h3>

Learn more about chemical equililbrium in:

brainly.com/question/24301138

8 0
1 year ago
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