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NYSTCE CST Chemistry (161) Practice Tests & Test Prep by Exam Edge - Review



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NYSTCE CST Chemistry - Reviews


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"Just wanted to say thanks for helping me pass the NYSTCE CST exams! Your practice tests and especially your explanations are great. Theygave me the confidence I needed! Now I can student teach this fall. I'm so glad I found your site!"

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See why our users from 154 countries love us for their exam prep! Including 85 reviews for the NYSTCE CST Chemistry exam.

Exam Edge is an industry leader in online test prep. We work with institutional partners to offer a wide array of practice tests that will help you prepare for your big exam. No matter how niche your field of interest might be, we're here to help you prepare for test day.

   Excellent -- Based on 85 reviews

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NYSTCE CST Chemistry - Test Reviews Sample Questions

A red balloon filled with Helium gas is enclosed by a blue balloon filled with an equal mass of Hydrogen. When the balloon reaches the maximum height, what is the ratio of the volume of the red balloon to the blue balloon? (Consider atomic wt of H2 = 2 and atomic wt of He = 4)

 

Correct Answer:
1:3
to solve the problem, we must first understand the relationship between the mass, molecular weight, and volume of gases under the same conditions of temperature and pressure.

since both helium (he) and hydrogen (h2) are gases, they follow the ideal gas law, which states that pv = nrt, where p is the pressure, v is the volume, n is the number of moles, r is the gas constant, and t is the temperature. at the same temperature and pressure, the volume of a gas is directly proportional to the number of moles (v = nrt/p, with r, t, and p being constant).

the number of moles of a gas can be found using the formula n = m/m, where m is the mass of the gas and m is the molar mass (molecular weight). given that both balloons are filled with an equal mass of gases and knowing the molecular weights (h2 = 2 g/mol, he = 4 g/mol), we can calculate the number of moles for each gas: - for hydrogen: n(h2) = m / 2 - for helium: n(he) = m / 4

since the mass m is the same for both gases, the number of moles of hydrogen (n(h2)) is twice that of helium (n(he)). this is because the molar mass of helium is twice that of hydrogen.

from the ideal gas law, and knowing that the number of moles of hydrogen is twice that of helium under the same conditions of temperature and pressure, it follows that the volume of hydrogen is also twice that of helium: - v(h2) = 2 * v(he)

now, the question specifies that a blue balloon encloses a red balloon, where the red balloon contains helium and the blue balloon contains hydrogen. however, there's an error in interpreting the setup of the balloons in the original explanation. the blue balloon is filled with an equal mass of hydrogen, not the sum of hydrogen and helium. therefore, the blue balloon contains only hydrogen, and its volume is twice that of the red balloon containing helium: - volume ratio (v(he) : v(h2)) = 1 : 2

thus, the volume of the red balloon (helium) to the blue balloon (hydrogen), when filled with an equal mass of each gas and considering the molar masses, is 1:2. this corrects the misunderstanding about the composition of gases in the blue balloon.