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jarptica [38.1K]
2 years ago
15

What dose the T-cell attack

Chemistry
1 answer:
MAXImum [283]2 years ago
5 0

Answer:

killer T-cell find and destroy infected cells that have been turned into virus-making factories

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A chemist uses 4.0 l of sulfuric acid solution to produce 3.2 gram of product. how much of the same sulfuric acid solution is ne
matrenka [14]
4 l ------ 3,2 g
x l ------ 8 g

x = 8 g × 4 l / 3,2 g = 10 l

Answer: 10 l of sulfuric acid is needed to produce 8 g of product.

:-) ;-)
3 0
3 years ago
Read 2 more answers
Many popular beverages are sold in two-kilo bottles. true or false
Molodets [167]
False. The answer is liter. kilo is the base (liter) times 1000. it would make no sense.
5 0
3 years ago
why do you think the experimenter conducted this experiment in a lab rather than in the natural world, where this phenomenon was
taurus [48]

Answer:

The experimenter observed this experiment in a lab rather than natural world because it might be dangerous to the atmosphere if he does the experiment in the natural world and it was still an hypothesis so that's why he did it in the lab.

5 0
3 years ago
HURRY I WILL GIVE YOU BRAINLIEST
Amiraneli [1.4K]

dim? im not so fluent in this but i did research yesterday

6 0
3 years ago
(Yield Problem)
alex41 [277]

Answer:

Percent Yield Fe  =  82.5%

Explanation:

The actual yield is the value produced after an experiment is conducted. The theoretical yield is the value calculated using the balanced chemical equation and atomic/molar masses.

To find the percent yield of iron (Fe), you need to (1) convert grams Al to moles Al (via atomic mass), then (2) convert moles Al to moles Fe (via mole-to-mole ratio from equation coefficients), then (3) convert moles Fe to grams Fe (via atomic mass), and then (4) calculate the percent yield. It is important to arrange the ratios in a way that allows for the cancellation of units. The final answer should have 3 sig figs to reflect the sig figs of the given values.

Atomic Mass (Mg): 24.305 g/mol

Atomic Mass (Fe): 55.845 g/mol

3 Mg + 2 FeCl₃ -----> 2 Fe + 3 MgCl₂

20.5 g Mg           1 mole              2 moles Fe            55.845 g
-----------------  x  -----------------  x  ----------------------  x  -----------------  =  
                           24.305 g           3 moles Mg             1 mole

=  31.4 g Fe

                                     Actual Yield
Percent Yield  =  ----------------------------------  x  100%
                                 Theoretical Yield

                               25.9 g Fe
Percent Yield  =  --------------------  x  100%
                               31.4 g Fe

Percent Yield  =  82.5%

5 0
2 years ago
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