Answer: 30. 7 moles SO3
31. 3 moles SO2 and 3 moles SO3
Explanation: To solve for this problem use the mole ratio of the substances involved in the reaction.
Solution for number 30:
3.5 moles O2 x 2 moles SO3 / 1 mole O2
= 7 moles SO3
31. 192 g SO2 x 1 mole SO2 / 64 g/ mol SO2
= 3 moles SO2
3 moles SO2 x 2 moles SO3 / 2 moles SO2
= 3 moles SO3
Answer:
D
Explanation:
The high jump of ionization energy indicates that we are trying to remove electron from noble gas configuration state.
The ionization energy data specifies that the Elements are from group 1 at period 3 or greater.
Removing the first electron require 496 kJ and the second ionization energy jump significantly due to the removal of electron from the noble gas configuration which is logical because electron try to maintain the especially stable state.
8) The gravitational force is a force of attraction between two objects. It can be expressed mathematically as:
F = G m₁*m₂/d² ------(1)
m₁ and m₂ are the masses of two interacting systems
d = distance between them
G = gravitational constant
Thus according to equation(1), the gravitational force is directly proportional to the mass of the objects. Greater the masses, stronger will be the force of attraction.
In this case, the distance (d) and the one of the masses i.e. mass of earth would be the same for both situations. However, since an elephant would weigh more than a human, the gravitational force will be stronger between an elephant and earth.
9) Since the masses of spheres is the same, the gravitational force between the red and blue spheres would be the same as well, provided the distance d remains constant.
Answer:
Explanation:
Hello.
In this case, since no information about the reacting hydrogen is given, we can assume that it completely react with the 28.0 g of acetylene to yield ethane. In such a way, via the 1:1 mole ratio between acetylene (molar mass = 26 g/mol) and ethane (molar mass = 30 g/mol), we compute the yielded grams, or the theoretical yield of ethane as shown below:
Hence, by knowing that the percent yield is computed via the actual yield (24.5 g) over the theoretical yield, we obtain:
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