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enyata [817]
2 years ago
8

Choose all options that apply . Which of the following are steps necessary to ensure patient safety ? a) Make sure that the medi

cation is dispensed in the same units in which it was prescribed. b ) Review any calculation questions with the pharmacist . Check to see if there's a better medication for the patient's problem. d) Dispense an extra dose to save the patient from having to return in case of loss or damage to one of the doses. Oe ) Compare the label on the medication with the order from the physician .
Chemistry
1 answer:
Tems11 [23]2 years ago
4 0

Answer:

c) Check to see if there's a better medication for the patient's problem.

d) Dispense an extra dose to save the patient from having to return in case of loss or damage to one of the doses.

e ) Compare the label on the medication with the order from the physician .

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PLEASE HELP!!
grandymaker [24]

Answer:

1. 136 °C.

2. 0.21 atm.

Explanation:

1. Determination of the new temperature in °C.

Initial volume (V1) = 1.35L

Final volume (V2) = 1.95L

Initial temperature (T1) = 283 K

Final temperature (T2) =...?

Using the Charles' law equation, the new temperature of the gas can be obtained as follow:

V1 /T1 = V2 /T2

1.35/283 = 1.95/T2

Cross multiply

1.35 × T2 = 283 × 1.95

1.35 × T2 = 551.85

Divide both side by 1.35

T2 = 551.85/1.35

T2 = 408.8 ≈ 409 K

Finally, we shall convert 409 K to °C. This can be obtained as follow:

T (°C) = T(K) – 273

T(K) = 409 K

T (°C) = 409 – 273

T (°C) = 136 °C

Therefore, the new temperature of the gas is 136 °C.

2. Determination of the new pressure.

Initial pressure (P1) = 1.34 atm

Initial volume (V1) = 267 mL

Final volume (V2) = 1.67 L

Final pressure (P2) =.?

Next, we shall convert 1.67 L to millilitres (mL). This can be obtained as follow:

1 L = 1000 mL

Therefore,

1.67 L = 1.67 L × 1000 mL / 1 L

1.67 L = 1670 mL

Therefore, 1.67 L is equivalent to 1670 mL.

Finally, we shall determine the new pressure of the gas as follow:

Initial pressure (P1) = 1.34 atm

Initial volume (V1) = 267 mL

Final volume (V2) = 1670 mL

Final pressure (P2) =.?

P1V1 = P2V2

1.34 × 267 = P2 × 1670

357.78 = P2 × 1670

Divide both side by 1670.

P2 = 357.78 / 1670

P2 = 0.21 atm.

Therefore, the new pressure of the gas is 0.21 atm.

3 0
3 years ago
Sonja and Jeremy performed several experiments to show how changes in temperature affected the volume of an inflated balloon. Th
ycow [4]

Answer:

They also showed the effects of pressure on volume if temperature stayed the same

Explanation:

They also showed the effects of pressure on volume if temperature stayed the same is the experiment that will provide an evidence for Boyle's law.

Boyle's law states that "the volume of a fixed mass of a gas varies inversely as the pressure changes, if the temperature is constant".

  • The law is an affirmation of what happens when there is a dynamics between pressure and volume if temperature is made constant.
  • So the experiment designed to investigate this proves and shows Boyle's law.
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a is the anwser

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