erperme rurgreming SECOND OUARTE RLV BUMMATNE ABBESBMENT IN QENFRAR. CHEMISTRY ? What is mole fraction in s ectutien? a. The number of moles of a sotuin divided by the fotat number of metes in the silition. b. The mase of s scitie difted thy the total mass of the saluticn c. The volume of e solute divided by the totat volume of the sotution The concentration of a solute in moles per hiter 2 Which of the following statemerits is true about mote fraction? a. Mole fraction is always tess thitit 4 . C. Mole fraction can be negative. b. Mole fraction is always greater than i. d. Mole fraction is a dimensionless quartity How is mole fraction calculated in a solution? a. Mass of solute / Volume of solution c. Moles of solute / Moles of soliution b. Moles of solute / Moles of solvent d. Moles of solute / Mass of solution A solution contains 10 moles of solute and 20 moles of solvent. What is the mole fraction of the solute? a. 0.5 b. 1.0 C. 2.0 d. 10.0 Which statement accurately describes the relationship between mole fraction and concentration? a. Mole fraction and concentration are the same thing. b. Mole fraction is always greater than concentration. c. Mole fraction is always less than concentration. d. Mole fraction and concentration are unrelated. What is the sum of the mole fractions of all components in a solution? a. 0 b. 1 c. 100 d. -1 How does the mole fraction of a solute change if more solvent is added to the solution? a. It increases. c. It remains the same. b. It decreases. d. It depends on the initial mole fraction of the solute. Which of the following is an example of a solution with a mole fraction of 0.75 ? a. A solution containing 1 mole of solute and 4 moles of solvent b. A solution containing 3 moles of solute and 1 mole of solvent c. A solution containing 75 grams of solute and 100 grams of solvent d. A solution containing 0.75 moles of solute and 1 mole of solvent What does a mole fraction of 1 mean? a. The solution is saturated. c. The solution is supersaturated. b. The solution is dilute. d. The solution is concentrated. How does the mole fraction of a solute change if more solute is added to the solution? a. It increases. c. It remains the same. b. It decreases. d. It depends on the initial mole fraction of the solute. How can we define of molarity? a. The amount of solute per unit volume of a solution b. The measure of the total number of particles in a solution c. The ratio of the mass of a solute to the volume of a solution d. The concentration of a solution expressed in terms of moles of solute per liter of solution Which formula is used to calculate molarity? a. M=( moles of solute )// (moles of solvent) b. M= (moles of solute)/(volume of solution in liters) c. M= (mass of solute)/(volume of solvent in liters) d. M=( mass of solute )//( moles of solvent)

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### Answer

<p><br />1. A<br />2. A, D<br />3. C<br />4. A<br />5. D<br />6. B<br />7. B<br />8. B<br />9. D<br />10. A<br />11. D<br />12. B

### Explanation

<p> <br />This question encompasses multiple critical topics in chemistry: mole fraction, its characteristics and computation, and the relation between mole fraction and concentration. It also delves into molarity and related calculations. <br /><br />1. Mole fraction is a method of expressing the concentration of an ingredient in a solution. It is the ratio of the moles of said ingredient to the total number of moles of all the constituents.<br />2. Many aspects of mole fraction are discussed here like its natural range (0 to 1), its attribute of being a dimensionless quantity, etc.<br />3. The proper formula for mole fraction revealed here accounts a correctly chosen pair of numerator and denominator from the several methods of various units presented.<br />4. Demonstrated here participant's understanding towards mole fraction through its practical computation reflecting its role as a proportion.<br />5. This question explicates the relationship (or lack thereof) between concentration and mole fraction. <br />6. The concept of the total sum of mole fractions in a solution being 1 is dabbed on.<br />7 & 10. These questions engage understanding on the variation in mole fraction due to changes in a solution's composition.<br />8. A selection of alternatives highlights some fundamental pitfalls to avoid when determining mole fractions.<br />9. Giving significance to a mole fraction of 1 shows the understanding of a solution's composition.<br />11 & 12. The concept and relevant calculated formula of molarity are offered for student's consideration.

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