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ss7ja [257]
4 years ago
7

A patient needs to be given exactly 1000 ml of a 5.0% (w/v) intravenous glucose solution. the stock solution is 55% (w/v). how m

any milliliters of the stock solution are needed to prepare the fluid for the iv bag?
Chemistry
1 answer:
LiRa [457]4 years ago
6 0
The patient needs 1000 ml of 5% (w/v) glucose solution
i.e  1000 ml x 5 g/ 100 ml 
where the stock solution is 55% (w/v) = 55 g / 100 ml  
So, 1000 ml x 5 g / 100 ml = V (ml) x 55 g / 100 ml 
V = 1000 x (5 / 100) / (55 / 100) = 5000 / 55 = 90.9 ml 
∴ the patient needs 90.9 ml of 55% (w/v) glucose solution

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Answer: The specific heat of the unknown metal is 0.897J/g^0C

Explanation:

The quantity of heat required to raise the temperature of a substance by one degree Celsius is called the specific heat capacity.

Q=m\times c\times \Delta T

Q = Heat absorbed=5040 Joules

m= mass of substance = 86.8 g

c = specific heat capacity = ?

Initial temperature of the water = T_i

Final temperature of the water = T_f

Change in temperature ,\Delta T=T_f-T_i=(64.7)^0C

Putting in the values, we get:

5040=86.8\times c\times 64.7^0C

c=0.897J/g^0C

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A mixture of 14.2 g of H2 and 36.7 g of Ar is placed in a 100.0 L container at
TiliK225 [7]

a) The total pressure of the system is  1.79 atm

b) The mole fraction and partial pressure of hydrogen is  0.89 and 1.59 atm respectively

c) The mole fraction and the partial pressure  of argon is 0.11 and 0.19 atm.

<h3>What is the total pressure?</h3>

We know tat we can be able to obtain the total pressure in the system by the use of the ideal gas equation. We would have from the equation;

PV = nRT

P = pressure

V = volume

n = Number of moles

R = gas constant

T = temperature

Number of moles of hydrogen = 14.2 g/2g = 7.1 moles

Number of moles of Argon = 36.7 g/40 g/mol

= 0.92 moles

Total number of moles =  7.1 moles + 0.92 moles = 8.02 moles

Then;

P = nRT/V

P = 8.02 * 0.082 * 273/100

P = 1.79 atm

Mole fraction of hydrogen = 7.1/8.02 = 0.89

Partial pressure of hydrogen =  0.89 * 1.79 atm

= 1.59 atm

Mole fraction of argon = 0.92 / 8.02

= 0.11

Partial pressure of argon = 0.11  *  1.79 atm

= 0.19 atm

Learn more about partial pressure:brainly.com/question/13199169

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