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sammy [17]
3 years ago
9

why I which activity would stimulate the human immune system to provide protection against an invasion by a microbe

Chemistry
1 answer:
Andrei [34K]3 years ago
6 0

The question is incomplete as it does not have the options which are:

(1) receiving antibiotic injections after surgery

(2) choosing a well-balanced diet and following it throughout life

(3) being vaccinated against chicken pox

(4) receiving hormones contained in mothers milk while nursing

Answer:

Being vaccinated against chicken pox

Explanation:

Vaccination is the procedure of giving the disease-causing germs which could be virus and bacteria in their dead or weakened state, some toxin, some proteins or some other molecules called a vaccine.

The benefit of providing vaccination is that the provided pathogen acts as an antigen and triggers the proactive immune response against the pathogen which helps in eradicating the main pathogen that has invaded the body.  The vaccination is used to treat the disease like chickenpox, measles, tetanus and many others.

Thus, the selected option is correct.

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Two moles of magnesium (Mg) and five moles of oxygen (O2) are placed in a
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First off, the chemical equation needs to be balanced. Since there are 2 oxygen atoms in the reactants, we must produce 2 moles of MgO, which means we need 2 moles of Mg, giving:
2Mg + O2 --> 2MgO
Therefore for a stoichiometric reaction where no reactant is left over, the number of moles of magnesium must be double that of oxygen. However, as seen, the molar ratio of magnesium to oxygen is 2:5, meaning oxygen is in large excess, and Magnesium is the limiting reactant. Therefore the answer is A.
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What volume of CH4(g), measured at 25oC and 745 Torr, must be burned in excess oxygen to release 1.00 x 106 kJ of heat to the su
anastassius [24]

Answer:

V=27992L=28.00m^3

Explanation:

Hello,

In this case, the combustion of methane is shown below:

CH_4+2O_2\rightarrow CO_2+2H_2O

And has a heat of combustion of −890.8 kJ/mol, for which the burnt moles are:

n_{CH_4}=\frac{-1.00x10^6kJ}{-890.8kJ/mol}= 1122.6molCH_4

Whereas is consider the total released heat to the surroundings (negative as it is exiting heat) and the aforementioned heat of combustion. Then, by using the ideal gas equation, we are able to compute the volume at 25 °C (298K) and 745 torr (0.98 atm) that must be measured:

PV=nRT\\\\V=\frac{nRT}{P}=\frac{1122.6mol*0.082\frac{atm*L}{mol*K}*298K}{0.98atm}\\\\V=27992L=28.00m^3

Best regards.

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